Fakir Mohan University, Balasorefmuniversity.nic.in/pdf/chem_2018.pdfRedox equations, Standard Electrode Potential and its application to inorganic reactions. Principles involved in

Syllabus and Scheme of Examination

for

B.Sc. Chemistry (Honours)

& B.Sc. Chemistry

Fakir Mohan University, Balasore

Under

Choice Based Credit System (CBCS)

(Applicable from the Academic Session 2016-17 onwards)

Choice Based Credit System in B.Sc. Courses of Chemistry (Honours & B.Sc. Chemistry, G.E,

AEC & SEC

1. B.Sc. (Pass & Honours) Degree course consists of six semesters in a consecutive of three

academic sessions from first admission. Each academic session consists of two semesters i.e.

odd semester & even semesters.

2. Marks, credit, no. of theory & lab papers for chemistry (Hons.) for six semesters are given

below.

Total Marks 2400 Total Papers-48

Total Credits 140

Honours Theory Papers 14 Marks 1400 Credits 84

Honours Lab Papers 14

DSE Theory Papers 4 400 24

DSE Lab Papers 4

GE Theory Papers 4 400 24

GE Lab Papers 4

AEC Theory Papers 2 100 4

SEC Theory Papers 2 100 4

2400 140

For Semester-I

Sl.No. Courses Paper Name Marks Credits Total Marks

1

AEC-I

MIL

Mid Sem-10

End Sem-40

2

50

2

HONS.

C-I

Inorganic Chem-I

Mid Sem-15

End Sem-60

4

100 3 Hons. C-I Lab. Inorganic Chem-I Lab Lab-25 2

4

Hons C-II

Physical Chem-I

Mid Sem-15

End Sem-60

4

100 5 Hons. C-II Lab Physical Chem-II Lab Lab-25 2

6

Generic Elective,

GE-I(Th.)

Mid Sem-15

End Sem-60

4

100 7 Generic Elective GE-I Lab Lab-25 2

Total Credits 20 350 Marks

For Semester-II


1

AEC-II

Environmental Science

Mid Sem-10

End Sem-40

2

50

2

HONS.

C-III Organic Chem-I

Mid Sem-15

End Sem-60

4

100 3 Hons. C-III Lab. Organic Chem-I Lab Lab-25 2

4

Hons C-IV

Physical Chem-II

Mid Sem-15

End Sem-60

4

100 5 Hons. C-IV Lab Physical Chem-II Lab Lab-25 2

6

Generic Elective-2

GE-2(Th.)

Mid Sem-15

End Sem-60

4

100 7 Generic Elective-2 GE-2 Lab Lab-25 2 Total Credits 20 350 Marks

3. Marks, Credit, number of theory & Lab papers for B.Sc. Chemistry students for six semesters

are given below.

Total Marks-2100

Total Credits-120

TotalPapers-42

1. Discipline specific courses for three subjects including chemistry 1200 marks, Each subject

400 marks.

TotalCredits-72 forChemistry-24Credits

For Chemistry-Theory Papers-04 400 marks

(DSC-2A, 2B, 2C & 2D), Lab Papers-04

2. DSE-600 marks, Each Subject-200 marks

Total Credits-36, for Chemistry-200 marks, for chemistry-12 credits

For Chemistry-(DSE-1 & DSE-2)

TheoryPapers-02 200 Marks

Lab Papers-02

3. Ability enhancement courses (Compulsory)

Two subjects-Two Theory Papers-100 marks

AEC-I=MIL/Communicative English

AEC-II=Environmental Science

Each Paper- 50 marks - 2 Credits

Total Credits-04

4. Skill Enhancement courses(SEC)

Subject- Chemistry- Four Theory papers-200 marks- Total Credits-08

Each paper – 50 marks – 2 Credits

Papers- SEC-I, SEC-2, SEC-3, SEC-4

For Semester-I


1

Chemistry DSC

(TH.)

DSC-2A

Mid Sem-15

End Sem-60

4

100 2 Chemistry DSC Lab. DSC-2A Lab. Lab-25 2

3

Other subject DSC

(Th)

DSC-1A Mid Sem-15

End Sem-60

4

100

4

Other subject DSC

Lab

DSC-1A Lab

Lab-25

2

5

Another subject

DSC (TH)

DSC-3A

Mid Sem-15

End Sem-60

4

100

6

Another Subject

DSC Lab

DSC-3A Lab

Lab-25

2

7 Generic Elective-2 GE-2 Lab Lab-25 2 50


For Semester-I


1

Chemistry DSC

(TH.)

DSC-2B

Mid Sem-15

End Sem-60

4

100 2 Chemistry DSC Lab. DSC-2B Lab. Lab-25 2

3

Other subject DSC

(Th)

DSC-1B

Mid Sem-15

End Sem-60

4

100

4

Other subject DSC

Lab

DSC-1B Lab

Lab-25

2

5

Another subject

DSC (TH)

DSC-3B

Mid Sem-15

End Sem-60

4

100

6

Another Subject

DSC Lab

DSC-3B Lab

Lab-25

2

7

AEC-2

Environmental Science

(Th)

Mid Sem-10

End Sem-40

2

50


4. Duration of odd semesters (SEM-1,3 & 5) is from June to November and even Semesters (SEMS-

2,4 & 6) is from December to May in each academic session.

5. Each theory paper consists of Mid Sem and End Sem Examinations.

6. Each lab paper will be held only in End Sem examinations.

7. Mid Sem Examinations of all theory papers of a semester will be conducted during the period of

that semester bythecollege. Markssecuredbyeachstudent ineachpaper will besent toUniversity

for computation.

8. EndSemexaminationsoftheorypapersandlabpaperswillbeconductedbytheUniversityatthe

end of respectivesemesters.

9. For eachtheory paper, marks for mid sem examination is -

Papers with Practical components – 15 marks

Papers without practical components- 10/20 marks

10. There shall be no mid sem examinations for lab papers.

11. Full marks for each thoey papers in end sem examinations is-

Papers with Practical components – 60 marks

Papers without practical components- 40/80 marks

12. Each theory paper of end sem examinations of Chemistry ( Hons., Pass, DSE, DSC & GE) papers

has four units. Students have to answer four questions out of four sets of alternative questions

covering all the units given in the examinations.

CORE COURSE ; SEMESTER- I B.SC.- CHEMISTRY( HONOURS )

CHEMISTRY-CC- I (Th.) : INORGANIC CHEMISTRY-I

Time – 3 hrs. F.M. – 100 [ 60( Sem) +15 (Int.) + 25 (Pr.) ](Credits: -04(Th.) +02(Pr.)

Lectures – 60 [ 40(Th.) + (Pr.)

Unit-I

ATOMIC STRUCTURE:

Bohr’s theory, its limitations and atomic spectrum of hydrogen atom. Wave mechanics: de

Broglie equation, Heisenberg’s Uncertainty Principle and its significance, Schrödinger’s

wave equation, significance of ψ and ψ2 . Quantum numbers and their significance. Normalized and orthogonal wave functions. Sign of wave functions. Radial and angular

wave functions for hydrogen atom. Radial and angular distribution curves. Shapes of s, p, d and f orbitals. Contour boundary and probability diagrams. Pauli’s Exclusion Principle,

Hund’s rule of maximum multiplicity, Aufbau’s principle and its limitations, Variation of

orbital energy with atomic number. (14 Lectures)

Unit-II

PERIODICITY OF ELEMENTS

Periodicity of Elements: s, p, d, f block elements, the long form of periodic table. Detailed

discussion of the following properties of the elements, with reference to s & p-block. (a)

Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective

nuclear charge in periodic table. (b) Atomic radii (van der Waals) (c) Ionic and crystal radii.

(d) Covalent radii (octahedral and tetrahedral) (e) Ionization enthalpy, Successive

ionization enthalpies and factors affecting ionization energy. Applications of ionization

enthalpy. (f) Electron gain enthalpy, trends of electron gain enthalpy. (g) Electronegativity,

Pauling’s/ Mulliken’s/ Allred Rachow’s/ and Mulliken-Jaffé’s electronegativity scales.

Variation of electronegativity with bond order, partial charge, hybridization, group

electronegativity. Sanderson’s electron density ratio. (16 Lectures)

Unit-III

CHEMICAL BONDING-I

(i) lonic bond: General characteristics, types of ions, size effects, radius ratio rule and its

limitations. Packing of ions in crystals. Born-Landé equation with derivation and

importance of Kapustinskii expression for lattice energy. Madelung constant, Born-Haber

cycle and its application, Solvation energy. (ii) Covalent bond: Lewis structure, Valence

Bond theory (Heitler-London approach). Energetics of hybridization, equivalent and non-

equivalent hybrid orbitals. Bent’s rule, Resonance and resonance energy, Molecular orbital

theory. Molecular orbital diagrams of diatomic and simple polyatomic molecules N2, O2,

C2, B2, F2, CO, NO, and their ions; HCl, BeF2, CO2, (idea of s-p mixing and orbital interaction to be given). Formal charge, Valence shell electron pair repulsion theory

(VSEPR), shapes of simple molecules and ions containing lone pairs and bond pairs of

electrons, multiple bonding (σ and π bond approach) and bond lengths. Covalent character

in ionic compounds, polarizing power and polarizability. Fajan’s rules and consequences of

polarization. Ionic character in covalent compounds: Bond moment and dipole moment.

Percentage ionic character from dipole moment and electronegativity difference.

(16 Lectures)

Unit-IV

CHEMICAL BONDING:-II

(i) Metallic Bond: Qualitative idea of valence bond and band theories. Semiconductors and

insulators, defects in solids.

(ii) Weak Chemical Forces: van der Waals forces, ion-dipole forces, dipole-dipole interactions,

induced dipole interactions, Instantaneous dipole-induced dipole interactions. Repulsive

forces, Hydrogen bonding (theories of hydrogen bonding, valence bond treatment) Effects

of chemical force, melting and boiling points, solubility energetics of dissolution process.

(16 Lectures)

(iii) OXIDATION-REDUCTION:

Redox equations, Standard Electrode Potential and its application to inorganic reactions.

Principles involved in volumetric analysis to be carried out in class. (14 Lectures)

Reference Books: • Lee, J.D. Concise Inorganic Chemistry, ELBS, 1991. • Douglas, B.E. and Mc Daniel, D.H., Concepts & Models of Inorganic Chemistry, Oxford,

1970

• Atkins, P.W. & Paula, J. Physical Chemistry, Oxford Press, 2006.

• Day, M.C. and Selbin, J. Theoretical Inorganic Chemistry, ACS Publications 1962.

CHEMISTRY LAB- C- I LAB:

(F.M=25)

(Expt. -15, Viva Voce- 6 & Lab. Record- 4) Time – 3hrs

(A) Titrimetric Analysis

(i) Calibration and use of apparatus

(ii) Preparation of solutions of different Molarity/Normality of titrants

(B) Acid-Base Titrations

(i) Estimation of carbonate and hydroxide present together in mixture.

(ii) Estimation of carbonate and bicarbonate present together in a mixture.

(iii) Estimation of free alkali present in different soaps/detergents

(C) Oxidation-Reduction Titrimetry

(i) Estimation of Fe(II) and oxalic acid using standardized KMnO4 solution.

(ii) Estimation of oxalic acid and sodium oxalate in a given mixture.

Estimation of Fe(II) with K2Cr2O7 using internal (diphenylamine, anthranilic acid) and external indicator.

Reference text:

1. Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS.

CORE COURSE ; SEMESTER- I B.SC.- CHEMISTRY( HONOURS )

CHEMISTRY-CC- II (Th.) : : PHYSICAL CHEMISTRY- I


Lectures – 60 [ 40(Th.) + (Pr.)

Unit-I GASEOUS STATE

Kinetic molecular model of a gas: postulates and derivation of the kinetic gas equation;

collision frequency; collision diameter; mean free path and viscosity of gases, including

their temperature and pressure dependence, relation between mean free path and coefficient

of viscosity, calculation of σ from η; variation of viscosity with temperature and pressure.

Maxwell distribution and its use in evaluating molecular velocities (average, root mean

square and most probable) and average kinetic energy, law of equipartition of energy,

degrees of freedom and molecular basis of heat capacities.

Behaviour of real gases: Deviations from ideal gas behaviour, compressibility factor, Z, and

its variation with pressure for different gases. Causes of deviation from ideal behaviour. van

12 der Waals equation of state, its derivation and application in explaining real gas

behaviour, mention of other equations of state (Berthelot, Dietrici); virial equation of state;

van der Waals equation expressed in virial form and calculation of Boyle temperature.

Isotherms of real gases and their comparison with van der Waals isotherms, continuity of

states, critical state, relation between critical constants and van der Waals constants, law of

corresponding states. (18 Lectures)

Unit-II LIQUID STATE

(i) Qualitative treatment of the structure of the liquid state; Radial distribution function;

physical properties of liquids; vapour pressure, surface tension and coefficient of viscosity,

and their determination. Effect of addition of various solutes on surface tension and

viscosity. Explanation of cleansing action of detergents. Temperature variation of viscosity

of liquids and comparison with that of gases. Qualitative discussion of structure of water.

IONIC EQUILIBRIA- I

(ii) Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of

ionization, ionization constant and ionic product of water. Ionization of weak acids and

bases, pH scale, common ion effect; dissociation constants of mono-, di-and triprotic acids

(exact treatment). (12 Lectures)

Unit- III SOLID STATE

Nature of the solid state, law of constancy of interfacial angles, law of rational indices,

Miller indices, elementary ideas of symmetry, symmetry elements and symmetry

operations, qualitative idea of point and space groups, seven crystal systems and fourteen

Bravais lattices; X-ray diffraction, Bragg’s law, a simple account of rotating crystal method

and powder pattern method. Analysis of powder diffraction patterns of NaCl, CsCl and

KCl. Defects in crystals. Glasses and liquid crystals. (16 Lectures)

Unit-IV Ionic equilibria - II: Salt hydrolysis- calculation of hydrolysis constant, degree of hydrolysis and pH for different salts.

Buffer solutions; derivation of Henderson equation and its applications; buffer capacity, buffer

range, buffer action and applications of buffers in analytical chemistry and biochemical processes in

the human body. Solubility and solubility product of sparingly soluble salts – applications of

solubility product principle. Qualitative treatment of acid – base titration curves (calculation of pH

at various stages). Theory of acid–base indicators; selection of indicators and theirlimitations.

Multistage equilibria in polyelectrolyte systems; hydrolysis and hydrolysis constants.

(14 Lectures)

Reference Books: • Atkins, P. W. & Paula, J. de Atkin’s Physical Chemistry Ed., Oxford University Press 13(2006).

• Ball, D. W. Physical Chemistry Thomson Press, India (2007).

• Castellan, G. W. Physical Chemistry 4th Ed. Narosa (2004). • Mortimer, R. G. Physical

Chemistry 3rd Ed. Elsevier: NOIDA, UP (2009).

CHEMISTRY LAB-(C-II LAB)

(F.M=25)

(Expt. -15, Viva Voce- 6 &Lab. Record- 4) Time – 3hrs

1. Surface tension measurements.

a. Determine the surface tension by (i) drop number (ii) drop weight method.

b. Study the variation of surface tension of detergent solutions with concentration.

2. Viscosity measurement using Ostwald’s viscometer.

a. Determination of viscosity of aqueous solutions of (i) polymer (ii) ethanol and (iii) sugar

at room temperature.

b. Study the variation of viscosity of sucrose solution with the concentration of solute.

3. pH metry

a. Study the effect on pH of addition of HCl/NaOH to solutions of acetic acid, sodium

acetate and their mixtures.

b. Preparation of buffer solutions of different pH i. Sodium acetate-acetic acid ii.

Ammonium chloride-ammonium hydroxide

c. pH metric titration of (i) strong acid vs. strong base, (ii) weak acid vs. strong base.

d. Determination of dissociation constant of a weak acid.

Reference Books

• Khosla, B. D.; Garg, V. C. &Gulati, A. Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).

• Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry 8th

Ed.; McGraw-Hill: New York (2003).

• Halpern, A. M. &McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H.

Freeman & Co.: New York (2003).

CORE COURSE ; SEMESTER- II - B.SC.- CHEMISTRY( HONOURS )

CHEMISTRY-CC- III (Th.) : ORGANIC CHEMISTRY


Lectures – 60 [ 40(Th.) + (Pr.)

Unit -I BASICS OF ORGANIC CHEMISTRY:

Organic Compounds: Classification, and Nomenclature, Hybridization, Shapes of molecules,

Influence of hybridization on bond properties.

Electronic Displacements: Inductive, electromeric, resonance and mesomeric effects,

hyperconjugation and their applications; Dipole moment; Organic acids and bases; their

relative strength.

Homolytic and Heterolytic fission with suitable examples. Curly arrow rules, formal charges;

Electrophiles and Nucleophiles; Nucleophlicity and basicity; Types, shape and their relative

stability of Carbocations, Carbanions, Free radicals and Carbenes.

Introduction to types of organic reactions and their mechanism: Addition, Elimination and

Substitution reactions.

CARBON-CARBON SIGMA BONDS

Chemistry of alkanes: Formation of alkanes, Wurtz Reaction, Wurtz-Fittig Reactions, Free

radical substitutions: Halogenation -relative reactivity and selectivity.(12 Lectures)

Unit - II

STEREOCHEMISTRY

Fischer Projection, Newmann and Sawhorse Projection formulae and their

interconversions; Geometrical isomerism: cis–trans and, syn-anti isomerism E/Z notations

with C.I.P rules. Optical Isomerism: Optical Activity, Specific Rotation,

Chirality/Asymmetry, Enantiomers, Molecules with two or more chiral-centres,

Distereoisomers, meso structures, Racemic mixture and resolution. Relative and absolute

configuration: D/L and R/S designations. (18 Lectures)

Unit – III

CHEMISTRY OF ALIPHATIC HYDROCARBONS

A. Carbon-Carbon pi bonds:

Formation of alkenes and alkynes by elimination reactions, Mechanism of E1, E2, E1cb

reactions. Saytzeff and Hofmann eliminations.

Reactions of alkenes: Electrophilic additions their mechanisms (Markownikoff/ Anti

Markownikoff addition), mechanism of oxymercuration-demercuration,

hydroborationoxidation, ozonolysis, reduction (catalytic and chemical), syn and anti-

hydroxylation (oxidation). 1,2-and 1,4-addition reactions in conjugated dienes and, Diels-

Alder reaction; Allylic and benzylicbromination and mechanism, e.g. propene, 1-butene,

toluene, ethyl benzene. 15 Reactions of alkynes: Acidity, Electrophilic and Nucleophilic

additions. Hydration to form carbonyl compounds, Alkylation of terminal alkynes.

B. Cycloalkanes and Conformational Analysis

Types of cycloalkanes and their relative stability, Baeyer strain theory, Conformation

analysis of alkanes: Relative stability: Energy diagrams of cyclohexane: Chair, Boat and

Twist boat forms; Relative stability with energy diagrams. (18 Lectures)

Unit - IV

AROMATIC HYDROCARBONS

Aromaticity: Hückel’s rule, aromatic character of arenes, cyclic carbocations/carbanions

and heterocyclic compounds with suitable examples. Electrophilic aromatic substitution:

halogenation, nitration, sulphonation and Friedel-Craft’s alkylation/acylation with their

mechanism. Directing effects of the groups.(12 Lectures)

Reference Books:

• Morrison, R. N. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

• Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson

Education).

• Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural

Products), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

• Eliel, E. L. &Wilen, S. H. Stereochemistry of Organic Compounds; Wiley: London, 1994.

• Kalsi, P. S. Stereochemistry Conformation and Mechanism; New Age International, 2005.

CHEMISTRY LAB-C III LAB

(F.M=25)


1. Checking the calibration of the thermometer

2. Purification of organic compounds by crystallization using the following solvents:

a. Water

b. Alcohol

c. Alcohol-Water

3. Determination of the melting points of above compounds and unknown organic compounds

(Kjeldahl method and electrically heated melting point apparatus)

4. Effect of impurities on the melting point – mixed melting point of two unknown organic

compounds

5. Determination of boiling point of liquid compounds. (boiling point lower than and more

than 100 °C by distillation and capillary method)

6. Chromatography

a. Separation of a mixture of two amino acids by ascending and horizontal paper

chromatography

b. Separation of a mixture of two sugars by ascending paper chromatography

c. Separation of a mixture of o-and p-nitrophenol or o-and p-aminophenol by thin layer

chromatography (TLC)

Reference Books

• Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009)

• Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic Chemistry,

5th Ed., Pearson (2012)

CORE COURSE ; SEMESTER- II - B.SC.- CHEMISTRY( HONOURS )

CHEMISTRY-CC- IV (Th.) : PHYSICAL CHEMISTRY II


Lectures – 60 [ 40(Th.) + (Pr.)

Unit-I

CHEMICAL THERMODYNAMICS:

Intensive and extensive variables; state and path functions; isolated, closed and open

systems; zeroth law of thermodynamics.

First law: Concept of heat, q, work, w, internal energy, U, and statement of first law;

enthalpy, H, relation between heat capacities, calculations of q, w, U and H for reversible,

irreversible and free expansion of gases (ideal and van der Waals) under isothermal and

adiabatic conditions.

Thermochemistry: Heats of reactions: standard states; enthalpy of formation of molecules

and ions and enthalpy of combustion and its applications; calculation of bond energy, bond

dissociation energy and resonance energy from thermochemical data, effect of temperature

(Kirchhoff’s equations) and pressure on enthalpy of reactions. Adiabatic flame temperature,

explosion temperature. (14 Lectures)

Unit-II

Second Law: Concept of entropy; thermodynamic scale of temperature, statement of the

second law of thermodynamics; molecular and statistical interpretation of entropy.

Calculation of entropy change for reversible and irreversible processes.

Third Law: Statement of third law, concept of residual entropy, calculation of absolute

entropy of molecules.

Free Energy Functions: Gibbs and Helmholtz energy; variation of S, G, A with T, V, P;

Free energy change and spontaneity. Relation between Joule-Thomson coefficient and other

thermodynamic parameters; inversion temperature; Gibbs-Helmholtz equation; Maxwell 17

relations; thermodynamic equation of state. (14 Lectures)

Unit-III SYSTEMS OF VARIABLE COMPOSITION

Partial molar quantities, dependence of thermodynamic parameters on composition;

GibbsDuhem equation, chemical potential of ideal mixtures, change in thermodynamic

functions in mixing of ideal gases. CHEMICAL EQUILIBRIUM

Criteria of thermodynamic equilibrium, degree of advancement of reaction, chemical

equilibria in ideal gases, concept of fugacity. Thermodynamic derivation of relation

between Gibbs free energy of reaction and reaction quotient. Coupling of exoergic and

endoergic reactions. Equilibrium constants and their quantitative dependence on

temperature, pressure and concentration. Free energy of mixing and spontaneity;

thermodynamic derivation of relations between the various equilibrium constants Kp, Kc

and Kx. Le Chatelier principle (quantitative treatment); equilibrium between ideal gases

and a pure condensed phase. (18 Lectures)

Unit-IV

Solutions and Colligative Properties: Dilute solutions; lowering of vapour pressure,

Raoult’s and Henry’s Laws and their applications. Excess thermodynamic functions.

Thermodynamic derivation using chemical potential to derive relations between the four

colligative properties [(i) relative lowering of vapour pressure, (ii) elevation of boiling

point, (iii) Depression of freezing point, (iv) osmotic pressure] and amount of solute.

Applications in calculating molar masses of normal, dissociated and associated solutes in

solution. (14 Lectures)

Reference Books

• Peter, A. & Paula, J. de. Physical Chemistry 9th Ed., Oxford University Press (2011).

• Castellan, G. W. Physical Chemistry 4th Ed., Narosa (2004). • Engel, T. & Reid, P. Physical Chemistry 3rd Ed., Prentice-Hall (2012).

• McQuarrie, D. A. & Simon, J. D. Molecular Thermodynamics Viva Books Pvt. Ltd.: New

Delhi (2004).

• Assael, M. J.; Goodwin, A. R. H.; Stamatoudis, M.; Wakeham, W. A. & Will, S.

Commonly Asked Questions in Thermodynamics. CRC Press: NY (2011).

• Levine, I .N. Physical Chemistry 6th Ed., Tata McGraw Hill (2010).

• Metz, C.R. 2000 solved problems in chemistry, Schaum Series (2006

CHEMISTRY LAB- C IV LAB

(F.M=25)

(Expt. -15, Viva- 6 & Lab. Record- 4) Time – 3hrs

THERMOCHEMISTRY

(a) Determination of heat capacity of a calorimeter for different volumes using change of

enthalpy data of a known system (method of back calculation of heat capacity of

calorimeter from known enthalpy of solution or enthalpy of neutralization).

(b) Determination of heat capacity of the calorimeter and enthalpy of neutralization of

hydrochloric acid with sodium hydroxide.

(c) Calculation of the enthalpy of ionization of ethanoic acid.

(d) Determination of heat capacity of the calorimeter and integral enthalpy (endothermic

and exothermic) solution of salts.

(e) Determination of basicity/proticity of a polyprotic acid by the thermochemical method

in terms of the changes of temperatures observed in the graph of temperature versus time

for different additions of a base. Also calculate the enthalpy of neutralization of the first

step.

(f) Determination of enthalpy of hydration of copper sulphate.

(g) Study of the solubility of benzoic acid in water and determination of ∆H.

Reference Books

• Khosla, B. D.; Garg, V. C. &Gulati, A., Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).

• Athawale, V. D. &Mathur, P. Experimental Physical Chemistry New Age International:

New Delhi (2001).

GENERIC ELECTIVE; SEMESTER- I / III B.SC. CHEMISTRY(Inter-disciplinary) B.Sc. Hons. Students other than Chemistry Hons. will opt. four Chemistry GE Papers

CHEM. GE: I (tTh.)- ATOMIC STRUCTURE, BONDING, GENERAL ORGANIC

CHEMISTRY & ALIPHATIC HYDROCARBONS


Lectures – 60 [ 40(Th.) + (Pr.)

SECTION A: INORGANIC CHEMISTRY-1

Unit-I

Atomic Structure

(30 Periods)

Review of: Bohr’s theory and its limitations, dual behaviour of matter and radiation, de-

Broglie’s relation, Heisenberg Uncertainty principle. Hydrogen atom spectra. Need of a

new approach to Atomic structure.

What is Quantum mechanics? Time independent Schrodinger equation and meaning of

various terms in it. Significance of ψ and ψ2 , Schrödinger equation for hydrogen atom. Radial and angular parts of the hydogenicwavefunctions (atomic orbitals) and their

variations for 1s, 2s, 2p, 3s, 3p and 3d orbitals (Only graphical representation). Radial and angular nodes and their significance. Radial distribution functions and the concept of the

most probable distance with special reference to 1s and 2s atomic orbitals. Significance of

quantum numbers, orbital angular momentum and quantum numbers ml and ms. Shapes of

s, p and d atomic orbitals, nodal planes. Discovery of spin, spin quantum number (s) and

magnetic spin quantum number (ms).

Rules for filling electrons in various orbitals, Electronic configurations of the atoms.

Stability of half-filled and completely filled orbitals, concept of exchange energy. Relative

energies of atomic orbitals, Anomalous electronic configurations. (14 Lectures)

Unit-II

Chemical Bonding and Molecular Structure

Ionic Bonding: General characteristics of ionic bonding. Energy considerations in ionic

bonding, lattice energy and solvation energy and their importance in the context of stability

and solubility of ionic compounds. Statement of Born-Landé equation for calculation of

lattice energy, Born-Haber cycle and its applications, polarizing power and polarizability.

Fajan’s rules, ionic character in covalent compounds, bond moment, dipole moment and

percentage ionic character.

Covalent bonding: VB Approach: Shapes of some inorganic molecules and ions on the basis

of VSEPR and hybridization with suitable examples of linear, trigonal planar, square planar,

tetrahedral, trigonalbipyramidal and octahedral arrangements.

Concept of resonance and resonating structures in various inorganic and organic compounds.

MO Approach: Rules for the LCAO method, bonding and antibonding MOs and their

characteristics for s-s, s-p and p-p combinations of atomic orbitals, nonbonding combination

of orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods

(including idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and

NO+ . Comparison of VB and MO approaches. (16 Lectures)

Section B: Organic Chemistry-1

Unit- III (30 Periods)

Fundamentals of Organic Chemistry

Physical Effects, Electronic Displacements: Inductive Effect, Electromeric Effect, Resonance

and Hyperconjugation. Cleavage of Bonds: Homolysis and Heterolysis.

Structure, shape and reactivity of organic molecules: Nucleophiles and electrophiles.

Reactive Intermediates: Carbocations, Carbanions and free radicals.

Strength of organic acids and bases: Comparative study with emphasis on factors affecting

pK values. Aromaticity: Benzenoids and Hückel’s rule. (8 Lectures)

Stereochemistry

Conformations with respect to ethane, butane and cyclohexane. Interconversion of Wedge

Formula, Newmann, Sawhorse and Fischer representations. Concept of chirality (upto two

carbon atoms). Configuration: Geometrical and Optical isomerism; Enantiomerism,

Diastereomerism and Meso compounds). Threo and erythro; D and L; cis - trans

nomenclature; CIP Rules: R/ S (for upto 2 chiral carbon atoms) and E / Z Nomenclature (for

upto two C=C systems). (10 Lectures)

Unit- IV

Aliphatic Hydrocarbons

Functional group approach for the following reactions (preparations & reactions) to be

studied in context to their structure.

Alkanes: (Upto 5 Carbons). Preparation: Catalytic hydrogenation, Wurtz reaction, Kolbe’s

synthesis, from Grignard reagent. Reactions: Free radical Substitution: Halogenation.

Alkenes: (Upto 5 Carbons) Preparation: Elimination reactions: Dehydration of alkenes and

dehydrohalogenation of alkyl halides (Saytzeff’s rule); cis alkenes (Partial catalytic

hydrogenation) and trans alkenes (Birch reduction). Reactions: cis-addition (alk. KMnO4) and

trans-addition (bromine), Addition of HX (Markownikoff’s and anti-Markownikoff’s

addition), Hydration, Ozonolysis, oxymecuration-demercuration, Hydroboration-oxidation.

Alkynes: (Upto 5 Carbons) Preparation: Acetylene from CaC2 and conversion into higher

alkynes; by dehalogenation of tetra halides and dehydrohalogenation of vicinal-dihalides.

Reactions: formation of metal acetylides, addition of bromine and alkaline KMnO4,

ozonolysis and oxidation with hot alk. KMnO4. (12 Lectures)

Reference Books:

• J. D. Lee: A new Concise Inorganic Chemistry, E L. B. S.

• F. A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley.

• Douglas, McDaniel and Alexader: Concepts and Models in Inorganic Chemistry, John

Wiley.

• James E. Huheey, Ellen Keiter and Richard Keiter: Inorganic Chemistry: Principles of

Structure and Reactivity, Pearson Publication.

• T. W. Graham Solomon: Organic Chemistry, John Wiley and Sons.

• Peter Sykes: A Guide Book to Mechanism in Organic Chemistry, Orient Longman.

• E. L. Eliel: Stereochemistry of Carbon Compounds, Tata McGraw Hill.• I. L. Finar:

Organic Chemistry (Vol. I & II), E. L. B. S.

• R. T. Morrison & R. N. Boyd: Organic Chemistry, Prentice Hall. • ArunBahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand

GE- I- LAB: ATOMIC STRUCTURE, BONDING, GENERAL ORGANIC

CHEMISTRY & ALIPHATIC HYDROCARBONS

(F.M=25)


Section A: Inorganic Chemistry- Volumetric Analysis

1. Estimation of sodium carbonate and sodium hydrogen carbonate present in a mixture.

2. Estimation of oxalic acid by titrating it with KMnO4.

3. Estimation of water of crystallization in Mohr’s salt by titrating with KMnO4.

4. Estimation of Fe (II) ions by titrating it with K2Cr2O7 using internalindicator.

5. Estimation of Cu (II) ions iodometrically using Na2S2O3.

Section B:Organic Chemistry

1. Detection of extra elements (N, S, Cl, Br, I) in organic compounds (containing upto two

extra elements)

2. Separation of mixtures by Chromatography: Measure the Rf value in each case

(combination of two compounds to be given)

(a) Identify and separate the components of a given mixture of 2 amino acids (glycine,

aspartic acid, glutamic acid, tyrosine or any other amino acid) by paper

chromatography

(b) Identify and separate the sugars present in the given mixture by paper

chromatography.

Reference Books:

• Vogel’s Qualitative Inorganic Analysis, A.I. Vogel, Prentice Hall, 7th Edition. • Vogel’s Quantitative Chemical Analysis, A.I. Vogel, Prentice Hall, 6th Edition.

• Textbook of Practical Organic Chemistry, A.I. Vogel , Prentice Hall, 5th edition.

• Practical Organic Chemistry, F. G. Mann. & B. C. Saunders, Orient Longman, 1960.

GENERIC ELECTIVE; SEMESTER- II/ IV B.SC. CHEMISTRY(Inter-disciplinary

CHEM. GE: II (tTh.)- CHEMICAL ENERGETICS, EQUILIBRIA & FUNCTIONAL

ORGANIC CHEMISTRY


Lectures – 60 [ 40(Th.) + (Pr.)

( B.Sc. Hons. Students other than Chemistry Hons. will opt. 2 GE Papers )

Section A: Physical Chemistry-1(30 Lectures)

Unit-I

Chemical Energetics

Review of thermodynamics and the Laws of Thermodynamics.

Important principles and definitions of thermochemistry. Concept of standard state and

standard enthalpies of formations, integral and differential enthalpies of solution and dilution.

Calculation of bond energy, bond dissociation energy and resonance energy from

thermochemical data. Variation of enthalpy of a reaction with temperature – Kirchhoff’s

equation.Statement of Third Law of thermodynamics and calculation of absolute entropies of

substances. (10 Lectures)

Chemical Equilibrium:

Free energy change in a chemical reaction. Thermodynamic derivation of the law of chemical

equilibrium. Distinction between ΔG and ΔGo , Le Chatelier’s principle. Relationships

between Kp, Kc and Kx for reactions involving ideal gases. (8 Lectures)

Unit- II

Ionic Equilibria:

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of

ionization, ionization constant and ionic product of water. Ionization of weak acids and bases,

pH scale, common ion effect. Salt hydrolysis-calculation of hydrolysis constant, degree of

hydrolysis and pH for different salts. Buffer solutions. Solubility and solubility product of

sparingly soluble salts – applications of solubility product principle. (12 Lectures)

Section B: Organic Chemistry-2 (30 Lectures)

Unit- III



Aromatic hydrocarbons

Preparation (Case benzene): from phenol, by decarboxylation, from acetylene, from benzene

sulphonic acid.

Reactions: (Case benzene): Electrophilic substitution: nitration, halogenation and

sulphonation. Friedel-Craft’s reaction (alkylation and acylation) (upto 4 carbons on benzene).

Side chain oxidation of alkyl benzenes (upto 4 carbons on benzene). (8 Lectures)

Alkyl and Aryl Halides

Alkyl Halides (Upto 5 Carbons) Types of Nucleophilic Substitution (SN1, SN2 and SNi)

reactions.

Preparation: from alkenes and alcohols.

Reactions: hydrolysis, nitrite & nitro formation, nitrile &isonitrile formation. Williamson’s

ether synthesis: Elimination vs substitution.

Aryl Halides Preparation: (Chloro, bromo and iodo-benzene case): from phenol,

Sandmeyer&Gattermann reactions.

Reactions (Chlorobenzene): Aromatic nucleophilic substitution (replacement by –OH group)

and effect of nitro substituent. Benzyne Mechanism: KNH2/NH3 (or NaNH2/NH3).

Reactivity and Relative strength of C-Halogen bond in alkyl, allyl, benzyl, vinyl and aryl

halides. (8 Lectures)

Unit- IV

Alcohols, Phenols and Ethers (Upto 5 Carbons)

Alcohols: Preparation: Preparation of 10 , 20 and 30 alcohols: using Grignard reagent, Ester

hydrolysis, Reduction of aldehydes, ketones, carboxylic acid and esters.

Reactions: With sodium, HX (Lucas test), esterification, oxidation (with PCC, alk. KMnO4,

acidic dichromate, conc. HNO3). Oppeneauer oxidation Diols: (Upto 6 Carbons) oxidation of diols. Pinacol-Pinacolone rearrangement.

Phenols: (Phenol case) Preparation: Cumenehydroperoxide method, from diazonium salts.

Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation.

ReimerTiemann Reaction, Gattermann-Koch Reaction, Houben–Hoesch

Condensation,Schotten – Baumann Reaction.

Ethers (aliphatic and aromatic): Cleavage of ethers with HI.

Aldehydes and ketones (aliphatic and aromatic): (Formaldehye, acetaldehyde, acetone and

benzaldehyde)

Preparation: from acid chlorides and from nitriles.

Reactions – Reaction with HCN, ROH, NaHSO3, NH2-G derivatives. Iodoform test. Aldol

Condensation, Cannizzaro’s reaction, Wittig reaction, Benzoin condensation. Clemensen

reduction and Wolff Kishner reduction. Meerwein-PondorffVerley reduction.(14 Lectures)

Reference Books:

• T. W. Graham Solomons: Organic Chemistry, John Wiley and Sons.


• I.L. Finar: Organic Chemistry (Vol. I & II), E. L. B. S.

• R. T. Morrison & R. N. Boyd: Organic Chemistry, Prentice Hall.

• ArunBahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand.

• G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007).

• G. W. Castellan: Physical Chemistry 4th Edn. Narosa (2004).

• J. C. Kotz, P. M. Treichel& J. R. Townsend: General Chemistry CengageLening India Pvt.

Ltd., New Delhi (2009).

• B. H. Mahan: University Chemistry 3rd Ed. Narosa (1998).

• R. H. Petrucci: General Chemistry 5th Ed. Macmillan Publishing Co.: New York (1985).

GE- II LAB- LAB: CHEMICAL ENERGETICS, EQUILIBRIA & FUNCTIONAL

ORGANIC CHEMISTRY-I

(F.M=25)


Section A: Physical Chemistry

Thermochemistry

1. Determination of heat capacity of calorimeter for different volumes. 2. Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide.

3. Determination of enthalpy of ionization of acetic acid.

4. Determination of integral enthalpy of solution of salts (KNO3, NH4Cl).

5. Determination of enthalpy of hydration of copper sulphate.

6. Study of the solubility of benzoic acid in water and determination of ΔH.

Ionic equilibria

pH measurements

a) Measurement of pH of different solutions like aerated drinks, fruit juices, shampoos

and soaps (use dilute solutions of soaps and shampoos to prevent damage to the glass

electrode) using pH-meter.

b) Preparation of buffer solutions:

(i) Sodium acetate-acetic acid

(ii) Ammonium chloride-ammonium hydroxide Measurement of the pH of

buffer solutions and comparison of the values with theoretical values.

Section B: Organic Chemistry

1. Purification of organic compounds by crystallization (from water and alcohol) and

distillation. 2. Criteria of Purity: Determination of melting and boiling points.

3. Preparations: Mechanism of various reactions involved to be discussed. Recrystallisation,

determination of melting point and calculation of quantitative yields to be done.

(a) Bromination of Phenol/Aniline

(b) Benzoylation of amines/phenols

(c) Oxime and 2,4 dinitrophenylhydrazone of aldehyde/ketone

Reference Books

• A.I. Vogel: Textbook of Practical Organic Chemistry, 5th edition, Prentice-Hall.

• F. G. Mann & B. C. Saunders, Practical Organic Chemistry, Orient Longman (1960).

• B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co

DISCIPLINE SPECIFIC CORE ; Semester I- B.SC. CHEMISTRY

CHEM. : DSC-1/2/3-I (Th.) - ATOMIC STRUCTURE, BONDING,

GENERAL ORGANIC CHEMISTRY & ALIPHATIC HYDROCARBONS


Lectures – 60 [ 40(Th.) + (Pr.)

Unit- I

Section A: INORGANIC CHEMISTRY-1

ATOMIC STRUCTURE

(30 Periods)

Review of: Bohr’s theory and its limitations, dual behaviour of matter and radiation, de-

Broglie’s relation, Heisenberg Uncertainty principle. Hydrogen atom spectra. Need of a new

approach to Atomic structure.What is Quantum mechanics? Time independent Schrodinger

equation and meaning of various terms in it. Significance of ψ and ψ2, Schrödinger equation

for hydrogen atom.Radial and angular parts of the hydogenicwavefunctions (atomic orbitals)

and their variations for 1s, 2s, 2p, 3s, 3p and 3d orbitals (Only graphical representation).

Radial and angular nodes and their significance. Radial distribution functions and the concept

of the most probable distance with special reference to 1s and 2s atomic orbitals. Significance

of quantum numbers, orbital angular momentum and quantum numbers mland ms. Shapes of

s, p and d atomic orbitals, nodal planes. Discovery of spin, spin quantum number (s) and

magnetic spin quantum number (ms).

Rules for filling electrons in various orbitals, Electronic configurations of the atoms. Stability

of half-filled and completely filled orbitals, concept of exchange energy. Relative energies of

atomic orbitals, Anomalous electronic configurations. (14 Lectures)

Unit- II

CHEMICAL BONDING AND MOLECULAR STRUCTURE

Ionic Bonding: General characteristics of ionic bonding. Energy considerations in ionic

bonding, lattice energy and solvation energy and their importance in the context of stability

and solubility of ionic compounds. Statement of Born-Landé equation for calculation of

lattice energy, Born-Haber cycle and its applications, polarizing power and polarizability.

Fajan’s rules, ionic character in covalent compounds, bond moment, dipole moment and

percentage ionic character.

Covalent bonding: VB Approach: Shapes of some inorganic molecules and ions on the basis

of VSEPR and hybridization with suitable examples of linear, trigonal planar, square planar,

tetrahedral, trigonalbipyramidal and octahedral arrangements.

Concept of resonance and resonating structures in various inorganic and organic compounds.

MO Approach: Rules for the LCAO method, bonding and antibonding MOs and their

characteristics for s-s, s-p and p-p combinations of atomic orbitals, nonbondingcombination

of orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods

(including idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and

NO+. Comparison of VB and MO approaches. (16 Lectures)

Unit- III

Section B: Organic Chemistry-1

FUNDAMENTALS OF ORGANIC CHEMISTRY (30 Periods)

Physical Effects, Electronic Displacements: Inductive Effect, ElectromericEffect,Resonance

and Hyperconjugation. Cleavage of Bonds: Homolysis and Heterolysis.

Structure, shape and reactivity of organic molecules: Nucleophiles and electrophiles.

Reactive Intermediates: Carbocations, Carbanions and free radicals.

Strength of organic acids and bases: Comparative study with emphasis on factorsaffecting pK

values. Aromaticity: Benzenoids and Hückel’s rule. (08 Lectures)

Stereochemistry

Conformations with respect to ethane, butane and cyclohexane. Interconversion of Wedge

Formula, Newmann, Sawhorse and Fischer representations. Concept of chirality(upto two

carbon atoms). Configuration: Geometrical and Optical isomerism;Enantiomerism,

Diastereomerism and Meso compounds). Threo and erythro; D and L; cis - trans

nomenclature; CIP Rules: R/ S (for upto 2 chiral carbon atoms) and E / Z Nomenclature (for

upto two C=C systems). (10 Lectures)

Unit- IV

ALLIPHATIC HYDROCARBONS



Alkanes: (Upto 5 Carbons). Preparation: Catalytic hydrogenation, Wurtz reaction,Kolbe’s

synthesis, from Grignard reagent. Reactions: Free radical Substitution: Halogenation.

Alkenes: (Upto 5 Carbons) Preparation: Elimination reactions: Dehydration of alkenes and

dehydrohalogenation of alkyl halides (Saytzeff’s rule); cis alkenes (Partial catalytic

hydrogenation) and trans alkenes (Birch reduction). Reactions: cis-addition (alk. KMnO4)

and trans-addition (bromine), Addition of HX (Markownikoff’s and anti-Markownikoff’s

addition), Hydration, Ozonolysis, oxymecuration-demercuration, Hydroboration- oxidation.

Alkynes: (Upto 5 Carbons) Preparation: Acetylene from CaC2 and conversion intohigher

alkynes; by dehalogenation of tetra halides and dehydrohalogenation of vicinal-dihalides.

Reactions: formation of metal acetylides, addition of bromine and alkaline

KMnO4,ozonolysis and oxidation with hot alk. KMnO4. (12 Lectures)

References Books:

• J. D. Lee: A new Concise Inorganic Chemistry, E L. B. S.

• F. A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley.

• Douglas, McDaniel and Alexader: Concepts and Models in Inorganic Chemistry,

• James E. Huheey, Ellen Keiter and Richard Keiter: Inorganic Chemistry: Principles of

Structure and Reactivity, Pearson Publication.

• T. W. Graham Solomon: Organic Chemistry, John Wiley and Sons.

• Peter Sykes: A Guide Book to Mechanism in Organic Chemistry, Orient

• E. L. Eliel: Stereochemistry of Carbon Compounds, Tata McGraw Hill.

• I. L. Finar: Organic Chemistry (Vol. I & II), E. L. B. S.


• ArunBahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand

CHEMISTRY LAB: DSC-1/2/3-I LAB: ATOMIC STRUCTURE,

BONDING, GENERAL ORGANIC CHEMISTRY & ALIPHATIC HYDROCARBONS

(F.M=25)


SECTION A: INORGANIC CHEMISTRY - VOLUMETRIC ANALYSIS

1. Estimation of sodium carbonate and sodium hydrogen carbonate present in a mixture.

2. Estimation of oxalic acid by titrating it with KMnO4.

3. Estimation of water of crystallization in Mohr’s salt by titrating with KMnO4.

4. Estimation of Fe (II) ions by titrating it with K2Cr2O7 using internal indicator.

5. Estimation of Cu (II) ions iodometrically using Na2S2O3.

SECTION B: ORGANIC CHEMISTRY

1. Detection of extra elements (N, S, Cl, Br, I) in organic compounds (containing upto

2. Separation of mixtures by Chromatography: Measure the Rf value in each case

(combination of two compounds to be given)

(a) Identify and separate the components of a given mixture of 2 amino acids (glycine,

aspartic acid, glutamic acid, tyrosine or any other amino acid) by paper chromatography.

(b) Identify and separate the sugars present in the given mixture by paperchromatography.

References Books:

• Vogel’s Qualitative Inorganic Analysis, A.I. Vogel, Prentice Hall, 7th Edition.

• Vogel’s Quantitative Chemical Analysis, A.I. Vogel, Prentice Hall, 6th Edition.

• Textbook of Practical Organic Chemistry, A.I. Vogel , Prentice Hall, 5th edition.

• Practical Organic Chemistry, F. G. Mann. & B. C. Saunders, Orient Longman,

DISCIPLINE SPECIFIC CORE ; Semester II- B.SC. CHEMISTRY

CHEM. : DSC-1/2/3-II (Th.) CHEMICAL ENERGETICS, EQUILIBRIA &

FUNCTIONAL ORGANIC CHEMISTRY


Lectures – 60 [ 40(Th.) + (Pr.)

SECTION A: PHYSICAL CHEMISTRY-1

Unit- I (30 Lectures)

Chemical Energetics

Review of thermodynamics and the Laws of Thermodynamics. Important principles and

definitions of thermochemistry. Concept of standard state and standard enthalpies of

formations, integral and differential enthalpies of solution and dilution. Calculation of bond

energy, bond dissociation energy and resonance energy from thermochemical data. Variation

of enthalpy of a reaction with temperature – Kirchhoff’s equation.

Statement of Third Law of thermodynamics and calculation of absolute entropies of

substances. (10 Lectures)

Chemical Equilibrium

Free energy change in a chemical reaction. Thermodynamic derivation of the law of

chemical equilibrium. Distinction between ΔG and ΔGo , Le Chatelier’s principle.

Relationships between Kp, Kc and Kx for reactions involving ideal gases. (8 Lectures)

Unit- II

Ionic Equilibria

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of

ionization, ionization constant and ionic product of water. Ionization of weak acids and bases,

pH scale, common ion effect. Salt hydrolysis-calculation of hydrolysis constant, degree of

hydrolysis and pH for different salts. Buffer solutions. Solubility and solubility product of

sparingly soluble salts – applications of solubility product principle. (12 Lectures)

SECTION B: ORGANIC CHEMISTRY-II

Unit- III (30 Lectures)



Aromatic hydrocarbons

Preparation (Case benzene): from phenol, by decarboxylation, from acetylene, from benzene

sulphonic acid.

Reactions: (Case benzene): Electrophilic substitution: nitration, halogenation and

sulphonation. Friedel-Craft’s reaction (alkylation and acylation) (upto 4 carbons on benzene).

Side chain oxidation of alkyl benzenes (upto 4 carbons on benzene). (8 Lectures)

Alkyl and Aryl Halides

Alkyl Halides(Upto 5 Carbons) Types of Nucleophilic Substitution (SN1, SN2 and SNi)

reactions.

Preparation: from alkenes and alcohols.

Reactions: hydrolysis, nitrite & nitro formation, nitrile &isonitrile formation. Williamson’s

ether synthesis: Elimination vs substitution.

Aryl Halides Preparation: (Chloro, bromo and iodo-benzene case): from phenol,

Sandmeyer&Gattermann reactions.

Reactions (Chlorobenzene): Aromatic nucleophilic substitution (replacement by –OH group)

and effect of nitro substituent. Benzyne Mechanism: KNH2/NH3 (or NaNH2/NH3).

Reactivity and Relative strength of C-Halogen bond in alkyl, allyl, benzyl, vinyl and aryl

halides. (8 Lectures)

Unit- IV

Alcohols, Phenols and Ethers (Upto 5 Carbons)

Alcohols: Preparation: Preparation of 10 , 20 and 30 alcohols: using Grignard reagent, Ester

hydrolysis, Reduction of aldehydes, ketones, carboxylic acid and esters.

Reactions: With sodium, HX (Lucas test), esterification, oxidation (with PCC, alk. KMnO4,

acidic dichromate, conc. HNO3). Oppeneauer oxidation Diols: (Upto 6 Carbons) oxidation of

diols. Pinacol-Pinacolone rearrangement.

Phenols: (Phenol case) Preparation: Cumenehydroperoxide method, from diazonium salts.

Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation. Reimer-

Tiemann Reaction, Gattermann-Koch Reaction, Houben–Hoesch Condensation, Schotten –

Baumann Reaction.

Ethers (aliphatic and aromatic): Cleavage of ethers with HI.

Aldehydes and ketones (aliphatic and aromatic): (Formaldehye, acetaldehyde, acetone and

benzaldehyde)

Preparation: from acid chlorides and from nitriles.

Reactions – Reaction with HCN, ROH, NaHSO3, NH2-G derivatives. Iodoform test. Aldol

Condensation, Cannizzaro’s reaction, Wittig reaction, Benzoin condensation. Clemensen

reduction and Wolff Kishner reduction. Meerwein-PondorffVerley reduction. (14

Lectures)Reference Books:

• T. W. Graham Solomons: Organic Chemistry, John Wiley and Sons.


• I.L. Finar: Organic Chemistry (Vol. I & II), E. L. B. S.


• ArunBahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand.

• G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007).

• G. W. Castellan: Physical Chemistry 4th Edn. Narosa (2004).

• J. C. Kotz, P. M. Treichel& J. R. Townsend: General Chemistry CengageLening India Pvt.

Ltd., New Delhi (2009).

• B. H. Mahan: University Chemistry 3rd Ed. Narosa (1998).

• R. H. Petrucci: General Chemistry 5th Ed. Macmillan Publishing Co.: New York (1985).

CHEMISTRY LAB- DSC-1/2/3 -II LAB: CHEMICAL ENERGETICS,

EQUILIBRIA & FUNCTIONAL ORGANIC CHEMISTRY

(F.M=25)



Thermochemistry

1. Determination of heat capacity of calorimeter for different volumes.

2. Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide.

3. Determination of enthalpy of ionization of acetic acid.

4. Determination of integral enthalpy of solution of salts (KNO3, NH4Cl).

5. Determination of enthalpy of hydration of copper sulphate.

6. Study of the solubility of benzoic acid in water and determination of ΔH.

Ionic equilibria

pH measurements

a) Measurement of pH of different solutions like aerated drinks, fruit juices, shampoos and

soaps (use dilute solutions of soaps and shampoos to prevent damage to the glass electrode)

using pH-meter.

b) Preparation of buffer solutions:

(i) Sodium acetate-acetic acid

(ii) Ammonium chloride-ammonium hydroxide

Measurement of the pH of buffer solutions and comparison of the values with theoretical

values.


1. Purification of organic compounds by crystallization (from water and alcohol) and

distillation.

2. Criteria of Purity: Determination of melting and boiling points.

3. Preparations: Mechanism of various reactions involved to be discussed. Recrystallisation,

determination of melting point and calculation of quantitative yields to be done.

(a) Bromination of Phenol/Aniline

(b) Benzoylation of amines/phenols

(c) Oxime and 2,4 dinitrophenylhydrazone of aldehyde/ketone

Reference Books

• A.I. Vogel: Textbook of Practical Organic Chemistry, 5th edition, Prentice-Hall.

• F. G. Mann & B. C. Saunders, Practical Organic Chemistry, Orient Longman (1960).

• B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co.

SEMESTER-III CC-5: INORGANIC CHEMISTRY-II

(Credits-6: Theory-4, Practical-2)-Max. Marks: 100

THEORY (Each class 1 hr.): Marks-75[60 (Sem) +15 (Int.)]

PRACTICAL (Each class 2 hrs.): Marks-25

Lectures: 60 (40 Theory + 20 Practical classes)

UNIT-I: General Principles of Metallurgy

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham

diagrams for reduction of metal oxides using carbon and carbon monoxide as reducing

agent. Electrolytic Re-duction, Hydrometallurgy. Methodsof puri_cation of metals:

Electrolytic process, Parting process,

van Arkel-de Boer process and Monds process, Zone re_ning. (8 Lectures)

Acids and Bases

Brnsted-Lowry concept of acid-base reactions, solvated proton, relative strength of acids,

types of

acid-base reactions, Lewis acid-base concept, Classi_cation of Lewis acids, Hard and Soft

Acids and

Bases (HSAB) Application of HSAB principle. (8 Lectures)

UNIT-II: Chemistry of s and p Block Elements-I

Inert pair effect, Relative stability of different oxidation states, diagonal relationship and

anomalous behaviour of first member of each group. Allotropy and catenation. Complex

formationtendencyof sandp blockelements. Hydrides andtheirclassification ionic,

covalent and interstitial. Basic beryllium acetate and nitrate. (14 Lectures)

UNIT-III: Chemistry of s and p Block Elements-II

Study of the following compounds with emphasis on structure, bonding, preparation,

properties and uses. Boric acid and borates, boron nitrides, borohydrides (diborane)

carboranesandgraphiticcompounds, silanes.Oxidesandoxoacidsof nitrogen,Phosphorus and

chlorine. Peroxo acids of sulphur, interhalogen compounds, polyhalide ions,

pseudohalogens and basic properties of halogens. (14 Lectures)

UNIT-IV: Noble Gases

Occurrence and uses, rationalization of inertness of noble gases, Clathrates; preparation and

proper-ties of XeF2;XeF4andXeF6; Nature of bondingin noble gas compounds (Valence bond

treatment and MO treatment for XeF2). Molecular shapes of noble gas compounds (VSEPR

theory). (8 Lectures)

Inorganic Polymers:

Typesof inorganicpolymers,comparisonwithorganicpolymers,synthesis,structural

aspects and applications of silicones and siloxanes. Borazines, silicates and phosphazenes,

and polysulphates. (8 Lectures)

Reference Books: Lee, J.D. Concise Inorganic Chemistry, ELBS, 1991.

Douglas, B.E; Mc Daniel, D.H. & Alexander, J.J. Concepts & Models ofInorganic Chemistry 3rd Ed., John Wiley Sons, N.Y. 1994.

Greenwood, N.N. & Earnshaw. Chemistry of the Elements, Butterworth-Heinemann. 1997.

Cotton,F.A.&Wilkinson, G.AdvancedInorganicChemistry,Wiley,VCH,1999.

Miessler, G. L. & Donald, A. Tarr. Inorganic Chemistry 4th Ed., Pearson, 2010.

Shriver & Atkins, Inorganic Chemistry 5th Ed.

PRACTICAL: CC-5 LAB.

(A) Iodo /Iodimetric Titrations

(i) Estimation of Cu(II) and K2Cr2O7using sodium thiosulphate solution (Iodimetrically).

(ii) Estimation of available chlorine in bleaching powder iodometrically.

(B) Inorganic preparations

(i) Cuprous chloride,Cu2Cl2: (ii) Preparation of manganese(III) phosphate, MnPO4:H2O:

(iii) Preparationof aluminium potassium sulphate K2SO4:Al2(SO4)2:24H2O(Potashalum).

Reference Books: Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS. 1978

CC-6: ORGANIC CHEMISTRY-II


THEORY(Eachclass1hr.): Marks-75 [60 (Sem) +15 (Int.)]


Lectures:60(40Theory+ 20Practicalclasses)

UNIT-I: Chemistry of Halogenated Hydrocarbons

Alkyl halides: Methods of preparation, nucleophilic substitution reactions SN1, SN2 and SNi

mech-anisms with stereochemical aspects and effect of solvent etc.; nucleophilic

substitution vs. elimination. Aryl halides: Preparation, including preparation from diazonium

salts, nucleophilic aromatic substitution; SNAr, Benzyne mechanism. Relative reactivity of

alkyl, allyl/benzyl, vinyl and arylhalides towards nucleophilic substitution reactions.

Organometallic compounds of Mg and Li Use in synthesis of organic compounds. (16

Lectures)

UNIT-II: Alcohols, Phenols, Ethers and Epoxides

Alcohols: preparation, properties and relative reactivity of 1, 2, 3 alcohols, Bouvaelt-Blanc

Re-duction;Preparation andproperties of glycols: Oxidation byperiodicacid and lead

tetraacetate, Pinacol-Pinacolone rearrangement; Phenols: Preparation and properties;

Acidity and factors effecting it, Ring substitution reactions, eimerTiemann and

KolbesSchmidtReactions,FriesandClaisen rearrangementswithmechanism;Ethersand

Epoxides: Preparationandreactionswithacids. Reactionsof epoxideswithalcohols,

ammonia derivatives and LiAlH4 (16 Lectures)

UNIT-III: Carbonyl Compounds

Structure, reactivity and preparation: Nucleophilic additions, Nucleophilic addition-

elimination reactions with ammonia derivatives with mechanism; Mechanisms of Aldol and

Benzoincondensation,Knoevenagel condensation,Perkin,CannizzaroandWittigreaction,

Beckmann rearrangements,haloform reaction and Baeyer Villiger oxidation, - substitution

reactions, oxidations and reductions (Clemmensen, Wol_-Kishner, LiAlH4, NaBH4, MPV.;

Addition reactions of unsaturated carbonyl

compounds: Michael addition. Active methylene compounds: Keto-enol tautomerism.

Preparation and synthetic applications of diethyl malonate and ethyl acetoacetate. (14

Lectures)

UNIT-IV: Carboxylic Acids and their Derivatives

Preparation, physical properties and reactions of monocarboxylic acids: Typical reactions of

dicar-boxylic acids, hydroxy acids and unsaturated acids: succinic, lactic, malic, tartaric,

citric,maleicandfumaricacids;Preparationandreactionsofacidchlorides, anhydrides,

esters and amides; Compar-ative study of nucleophilic sustitution at acyl group -Mechanism

of acidic and alkaline hydrolysis of esters, Claisen condensation, Dieckmann and

Reformatsky reactions, Hofmann-bromamide degradation and Curtius rearrangement. (10

Lectures)

Sulphur containing compounds

Preparation and reactions of thiols, thioethers. (4 Lectures)

Reference Books: Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd.

(Pearson Education).

Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc.


1. Functional group tests for alcohols, phenols, carbonyl and carboxylic acid group.

2. Organic preparations:

(i) Acetylation of one of the following compounds: amines (aniline, o-, m-, p-toluidines and

o-, m-,p-anisidine) andphenols (-naphthol, vanillin, salicylic acid) byany one method:

(a) Using conventional method.

(b) Using green approach.

(ii) Benzolyation of one of thefollowingamines (aniline,o-, m-,p- toluidines ando-,m-,p-

anisidine) and one of the following phenols (-naphthol, resorcinol, p-cresol) by Schotten-

Baumann reaction.

(iii) Bromination of any one of the following:

(a) Acetanilide by conventionalmethods.

(b) Acetanilide using green approach (Bromate-bromide method).

(iv) Nitration of any one of the following:

(a) Acetanilide/nitrobenzene by conventionalmethod.

(b) Salicylic acid by green approach (using ceric ammonium nitrate).

The above derivatives should be prepared using 0.5-1gm. of the organic compound. The

solid samples must be collected and may be used for recrystallization, melting point and

TLC.

Reference Books: Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009).

Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic Chemistry, 5th Ed., Pearson (2012).

Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry:

Preparation and Quantitative Analysis, University Press (2000).

Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic Chemistry: Qualitative

Analysis, University Press (2000).

CC-7: PHYSICAL CHEMISTRY-III




Lectures:60 (40Theory+ 20Practicalclasses))

UNIT-I:Phase Equilibria-I

Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for

nonreactive and reactive systems; Clausius-Clapeyron equation and its applications to solid-

liquid, liquidvapour and solid-vapour equilibria, phase diagram for one component systems,

with applications (H2O and sulphur system).Phase diagramsforsystems of solid-liquid

equilibria involving eutectic, congruent and incongruent melting points, solid solutions (Pb-

Ag system, desilverisation of lead)

(14 Lectures)

UNIT-II: Phase Equilibria-II

Three component systems, water-chloroform-acetic acid system, triangular plots. Binary

solutions: Gibbs-Duhem-Margules equation, its derivation and applications to fractional

distillation of binary miscible liquids (ideal and non-ideal), azeotropes, partial miscibility of

liquids, CST,misciblepairs, steam distillation. Nernst distribution law: its derivation and

applications. (14 Lectures)

UNIT-III: Chemical Kinetics

Orderandmolecularityof a reaction, ratelaws intermsof theadvancement of a reaction,

differential and integrated form of rate expressions up to second order reactions,

experimental methods of the determination of orders, kinetics of complex reactions

(integrated rate expressions up to first order only): (i) Opposing reactions (ii) parallel

reactions and (iii) consecutive reactions and their differential rate equations (steady-state

approximation in reaction mechanisms) (iv) chain reactions.

Temperature dependence of reaction rates; Arrhenius equation; activation energy. Collision

theory of reaction rates, qualitative treatment of the theory of absolute reaction rates. (18

Lectures)

UNIT-IV: Catalysis

Typesof catalyst, specificityandselectivity,mechanismsof catalyzed reactionsatsolid

surfaces; effect of particle size and effciency of nanoparticles ascatalysts. Enzyme catalysis,

Michaelis-Menten mechanism, acid-base catalysis. (8 Lectures)

Surface chemistry

Physical adsorption,chemisorption, adsorptionisotherms(Langmuir, Freundlich andGibbs

isotherms), nature of adsorbed state. (6 Lectures)

Reference Books: PeterAtkins& Julio De Paula, Physical Chemistry 9th Ed.,Oxford University Press

(2010).

Castellan, G. W. Physical Chemistry, 4th Ed., Narosa (2004).

McQuarrie, D. A. & Simon, J. D., Molecular Thermodynamics, Viva Books Pvt. Ltd.:

New Delhi (2004).

Engel, T. & Reid, P. Physical Chemistry 3rd Ed., Prentice-Hall (2012).

Assael, M. J.; Goodwin, A. R. H.; Stamatoudis, M.; Wakeham, W. A. & Will, S.

Commonly Asked Questions in Thermodynamics. CRC Press: NY (2011).

Zundhal, S.S. Chemistry concepts and applications Cengage India (2011).

Ball, D. W. Physical Chemistry Cengage India (2012).

Mortimer, R. G. Physical Chemistry 3rd Ed., Elsevier: NOIDA, UP (2009).

Levine,I.N.PhysicalChemistry6thEd.,TataMcGraw-Hill(2011).

Metz, C. R. Physical Chemistry 2nd Ed., Tata McGraw-Hill (2009).


I. Distribution of acetic/ benzoic acid between water and cyclohexane.

II. Studythe equilibrium of at least one of thefollowing reactions by the distribu-

tion method:

I2 (aq)+ I- I3- (aq) Cu2+(aq)+nNH3 Cu(NH3)n:

III. Study the kinetics of the following reactions.

(1) Integrated rate method:

a. Acid hydrolysis of methyl acetate with hydrochloric acid.

b. Saponification of ethyl acetate.

(2) Compare the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of methyl

acetate.

Adsorption

Verify the Freundlich and Langmuir isotherms for adsorption of acetic acid on activated

charcoal.

Reference Books: Khosla,B.D.; Garg, V. C.& Gulati, A.SeniorPractical Physical Chemistry, R.Chand&

Co. New Delhi (2011).

Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experimentsin Physical Chemistry 8th Ed.; McGraw-Hill: New York (2003).

Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H.


SEMESTER- IV

CC-8: INORGANIC CHEMISTRY-III




Lectures:60 (40Theory+ 20 Practicalclasses)

UNIT-I: Coordination Chemistry

Werners theory, valence bond theory (inner and outer orbital complexes), electroneutrality

principle and back bonding. Crystal field theory, measurement of CFSE weak and strong

fields, pairing energies, factors affecting the magnitude of 10 Dq in octahedral vs.

tetrahedral coordination, tetragonaldistortionsfromoctahedral geometry, Jahn-Teller

theorem, square planar geometry. Qualitative as affpect of ligand field and MOTheory.

IUPAC nomenclature of coordination compounds, isomerism in coordination compounds.

Stereochemistry of complexes with 4 and 6 coordination numbers. Chelate effect, Labile and

inert complexes. (20 Lectures)

UNIT-II: Transition Elements-I

General group trends with special reference to electronic configuration, colour, variable

valency, magnetic and catalytic properties, ability to form complexes. Stability of various

oxidation states and e.m.f. (Latimer & Bsworth diagrams). Difference between the first,

second and third transition series. (12 Lectures)

UNIT-III: Transition Elements-II

Chemistry of Ti, V, Cr Mn, Fe and Co in various oxidation states (excluding their metallurgy).

(12 Lectures)

UNIT-IV: Lanthanoids and Actinoids

Electronic configuration, oxidationstates, colour, spectralandmagneticproperties,

lanthanide con-traction, separation of lanthanides (ion-exchange method only). General

features of actinoids, separation of Np, Pm, Am from U. (6 Lectures)

Bioinorganic Chemistry

Metal ions present in biological systems, classification of elements according to their action

in bilogical system. Na/K-pump, carbonic anhydrase and carboxypeptidase. Excess and

deficiencyof some trace metals. Toxicity of metal ions (Hg, Pb, Cd and As), reasonsfor

toxicity, Use of chelating agents in medicine. Iron and its application in bio-systems,

Haemoglobin; Storage and transfer of iron. (10 Lectures)

Reference Books:

Purcell, K.F & Kotz, J.C. Inorganic Chemistry W.B. Saunders Co, 1977.

Huheey, J.E., Inorganic Chemistry, Prentice Hall, 1993.

Lippard, S.J. & Berg, J.M. Principles of Bioinorganic Chemistry Panima Publishing

Company 1994.

Cotton, F.A. &Wilkinson, G, Advanced Inorganic Chemistry. Wiley-VCH, 1999.

Basolo, F, and Pearson, R.C., Mechanisms of Inorganic Chemistry, John Wiley & Sons, NY, 1967.

Greenwood, N.N. & Earnshaw A., Chemistry of the Elements, Butterworth- Heinemann, 1997.


Gravimetric Analysis:

i. Estimation of nickel(II) using Dimethylglyoxime (DMG).

ii Estimation of copper as CuSCN. iii. Estimation of iron as Fe2O3 by precipitating iron as Fe(OH)3:

iv. Estimation of Al(III) by precipitating with oxine and weighing as Al(oxine)3 (aluminium

oxinate).Chromatography of metal ions

Principalsinvolvedin chromatographic separations. Paper chromatographic separation of

following metal ions:

i. Ni(II) and Co(II)

ii. Fe(III) and Al(III)

Reference Book: Vogel, A.I. A text book of Quantitative Analysis, ELBS 1986.

CC-9: ORGANIC CHEMISTRY-III





UNIT-I: Nitrogen Containing Functional Groups

Preparation and important reactions of nitro and compounds, nitriles. Amines: Effect of

substituent and solvent on basicity; Preparation and properties: Gabriel hthalimide

synthesis, Carbylamine reaction, Mannich reaction, Hoffmanns exhaustive methylation,

Hofmann-elimination reaction;Dis-tinctionbetween 1,2and 3amineswith Hinsberg

reagent and nitrous acid. (14 Lectures)

UNIT-II: Diazonium Salts

Preparation and their synthetic applications.Polynuclear Hydrocarbons Reactions of

naphthalene and anthracene Structure, Preparation and structure elucidation and im-

portant derivatives of naphthalene and anthracene. Polynuclear hydrocarbons. (12 Lectures)

UNIT-III: Heterocyclic Compounds

Classi_cation and nomenclature, Structure, aromaticity in 5-numbered and 6-membered

rings con-taining one heteroatom; Synthesis, reactions and mechanism of substitution

reactionsof: Furan, Pyrrole (Paal-Knorr synthesis, Knorrpyrrole synthesis, Hantzsch

synthesis), Thiophene, Pyridine (Hantzsch synthesis), Pyrimidine. Fischer indole synthesis

and Madelung synthesis, structure of

quinoline and isoquinoline. Derivatives of furan: Furfural and furoic acid (preparation only).

(18 Lectures)

UNIT-IV: Alkaloids

Naturaloccurrence, General structuralfeatures, Isolation andtheirphysiological action

Hoffmanns exhaustive methylation, Emdes modification, Structure elucidation and synthesis

of Hygrine and Nicotine. Medicinal importance of Nicotine, Hygrine, Quinine, Morphine,

Cocaine, and Reserpine. (8 Lectures)

Terpenes Occurrence, classi_cation, isoprene rule; Elucidationof stucture and synthesis of

Citral, Neral and -terpineol. (8 Lectures)

Reference Books: Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd.


Finar,I. L. Organic Chemistry (Volume 1),Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural Products), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

Acheson, R.M. Introduction to the Chemistry of Heterocyclic compounds, John Welly

& Sons (1976).

Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc.

Kalsi,P.S.TextbookofOrganicChemistry1stEd.,NewAgeInternational(P)Ltd.Pub.

Clayden, J.; Greeves, N.; Warren, S.; Wothers, P.; Organic Chemistry, Oxford

University Press.

Singh,J.;Ali,S.M.&Singh,J.NaturalProductChemistry,PrajatiParakashan(2010).


1. Detection of extra elements (N, X, S).

2. Functional group test for nitro, amine and amide groups.

3. Qualitative analysis of unknown organic compounds containing simple functional groups

(alcohols, carboxylic acids, phenols and carbonyl compounds).

Reference Books: Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009).

Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic

Chemistry, 5th Ed., Pearson (2012).

Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry: Preparation and Quantitative Analysis, University Press (2000).

Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic Chemistry: Qualitative


CC-10: PHYSICAL CHEMISTRY-IV





UNIT-I: Conductance-I

Arrhenius theory of electrolytic dissociation. Conductivity, equivalent and molar

conductivity and their variation with dilution for weak and strong electrolytes. Molar

conductivity at infinite dilution. Kohlrausch law of independent migration of ions. Debye-

Hckel-Onsager equation, Wien effect, Debye-Falkenhagen effect, Waldens rules. (12

Lectures)

UNIT-II: Conductance-II

Ionic velocities, mobilities and their determinations, transference numbers and their

relation to ionic mobilities, determination of transference numbers using Hittorf and Moving

Boundary methods. Applications of conductance measurement: (i) degree of dissociation of

weak electrolytes, (ii)ionic productof water (iii) solubilityand solubilityproductof sparingly

soluble salts, (iv) conductometric titrations, and (v) hydrolysis constants of salts. (16

Lectures)

UNIT-III: Electrochemistry-I

Quantitative aspects of Faradays laws of electrolysis, rules of oxidation/reduction of ions

based on half-cellpotentials, applications of electrolysis in metallurgy and industry.

Chemical cells, reversible and irreversible cells with examples. Electromotive force of a cell

and itsmeasurement, Nernst equation; Standard electrode (reduction) potential and its

application to diferent kinds of half- cells. Application of EMF measurements in determining

free energy, enthalpyand entropyof a cell reaction, (ii)equilibrium constants, and (iii) pH

values, using hydrogen, quinone-hydroquinone, glass electrodes. (18 Lectures)

UNIT-IV: Electrochemistry-II

Concentration cells with and without transference, liquid junction potential; determination

of activity coeficients and transference numbers. Qualitative discussion of potentiometric

titrations(acid-base,redox, precipitation).Electricalpropertiesofatomsandmolecules

Basic ideas of electrostatics, Electrostatics of dielectric media. Clausius-Mosotti equation

and Lorenz-Laurentz equation (no

derivation), Dipole moment and molecular polarizabilities and their measurements. (14

Lectures)

Reference Books: Atkins,P.W&Paula,J.D.PhysicalChemistry,9thEd.,OxfordUniversityPress(2011).

Castellan, G. W. Physical Chemistry 4th Ed., Narosa (2004).

Mortimer, R. G. Physical Chemistry 3rd Ed., Elsevier: NOIDA, UP (2009).

Barrow, G. M., Physical Chemistry 5th Ed., Tata McGraw Hill: New Delhi (2006).

Engel, T. & Reid, P. Physical Chemistry 3rd Ed., Prentice-Hall (2012).

Rogers, D. W. Concise Physical Chemistry Wiley (2010).Silbey, R. J.; Alberty, R. A. &

Bawendi, M. G. Physical Chemistry 4th Ed., JohnWiley & Sons, Inc. (2005).


Conductometry

I. Determination of cell constant.

II. Determination of equivalent conductance, degree of dissociation and dissociation

constant of a weak acid.

III. Perform the following conductometric titrations:

i. Strong acid vs. strong base

ii. Weak acid vs. strong base

iii. Strongacidvs.weakbase

Potentiometry

I. Perform the following potentiometric titrations:

i. Strongacidvs.strongbase

ii. Weakacid vs.strongbase

iii. Dibasic acid vs. strong base

Reference Books: Khosla,B.D.;Garg,V.C.&Gulati, A. Senior Practical Physical Chemistry, R.Chand&

Co.: New Delhi(2011).

Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experimentsin Physical Chemistry

8th Ed.; McGraw-Hill: New York (2003).

Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H.


SKILL ENHANCEMENT COURSES (SEC) SEMESTER- IV

SEC-II: PESTICIDE CHEMISTRY

(Credits: 02)- Max. Marks: 50 [40 (Sem) +10 (Int.)]

30 Lectures( Each Lecture 1 hr.)

General introduction to pesticides (natural and synthetic), benefits and adverse effects,

changing concepts of pesticides, structure activity relationship, synthesis and technical

manufacture and uses of representative pesticides in the following classes: Organochlorines

(DDT, Gammexene,); Organophosphates (Malathion, Parathion ); Carbamates (Carbofuran

and carbaryl); Quinones (Chloranil), Anilides (Alachlor and Butachlor).

Practical To calculate acidity/alkalinity in given sample of pesticide formulations as per BIS

speci_cations.

Preparation of simple organophosphates, phosphonates and thiophosphates.

Reference Book:

R. Cremlyn: Pesticides, John Wiley.

SEMESTER-III

DSC-1/2/3-III(2C): SOLUTIONS,PHASE EQUILIBRIUM,

CONDUCTANCE, ELECTROCHEMISTRY & FUNCTIONAL

GROUP ORGANIC CHEMISTRY-II

(Credits:6 Theory-04, Practicals-02)

THEORY (Each class 1 hour):75 Marks[60 (Sem) +15 (Int.)]

PRACTICAL (Each class 2 hours):25 Marks

Lectures: 60(40 Theory + 20 Practical classes)

Section A: Physical Chemistry-2 (30 Lectures)

UNIT-I: Solutions

Thermodynamics of ideal solutions: Ideal solutions and Raoults law, deviations from Raoults

law non-ideal solutions. Vapour pressure-composition and temperaturecomposition curves

of ideal and non-ideal solutions. Distillation of solutions. Lever rule. Azeotropes.Partial

miscibility of liquids: Critical solution temperature; effect of impurity on partial miscibility of

liquids. Immiscibility of liquids- Principle of steam distillation. Nernst distribution law and its

applications, solvent extraction. (8 Lectures)

Phase Equilibrium

Phases, components and degrees of freedom of a system, criteria of phase equilibrium.

Gibbs Phase Rule and its thermodynamic derivation. Derivation of Clausius Clapeyron

equation and its importance in phase equilibria. Phase diagrams of one-component systems

(water and sulphur) and two component systems involving eutectics, congruent and

incongruent melting points (lead-silver, FeCl3 -H2O and Na-K only). (7 Lectures).

UNIT-II: Conductance

Conductivity, equivalentandmolarconductivityandtheirvariationwithdilutionforweak

and strong electrolytes. Kohlrausch law of independent migration of ions. Transference

number and its experimental determination using Hittorf and Moving boundary methods.

Ionic mobility. Applications of conductance measurements: determination of degree of

ionization of weak electrolyte, solubility and solubility products of sparingly soluble salts,

ionic product of water, hydrolysis constant of a salt. Conductometric titrations (only acid-

base). (7 Lectures)

Electrochemistry

Reversibleandirreversiblecells.ConceptofEMFofacell.MeasurementofEMFof acell.

Nernstequation and its importance. Types of electrodes. Standard electrode potential.

Electrochemical series. Thermodynamics of a reversible cell, calculation of thermodynamic

properties: G,Hand Sfrom EMFdata.Calculationof equilibrium constantfrom EMFdata.

Concentration cells with transference and without transference. Liquid junction potential

and salt bridge. pHdetermination using hydrogen electrode and quinhydrone electrode.

Potentiometric titrations -qualitative treat-ment (acid-base and oxidation-reduction only). (8

Lectures)

Section B: Organic Chemistry-3 (30 Lectures)

UNIT-III: Functional group approach for the following reactions (preparations & reactions) to

be studied in context to their structure.

Carboxylicacidsandtheirderivatives.

Carboxylicacids(aliphaticandaromatic)

Preparation: Acidic and Alkaline hydrolysis of esters.

Reactions: Hell Vohlard - Zelinsky Reaction.

Carboxylic acid derivatives (aliphatic): (Upto 5 carbons)

Preparation: Acid chlorides, Anhydrides, Esters and Amides from acids and their

interconversion.

Reactions: Comparative study of nucleophilicity of acyl derivatives. Reformatsky Reaction,

Perkin condensation. (6Lectures).

Amines and Diazonium Salts

Amines (Aliphatic and Aromatic): (Upto 5 carbons) Preparation: from alkyl halides, Gabriels

Ph-thalimide synthesis, Hofmann bromamide reaction. Reactions: Hofmann vs. Saytze_

elimination,Carbylaminetest,Hinsbergtest,withHNO2,SchottenBaumannReaction.

Electrophilic substi-tution (case aniline): nitration, bromination, sulphonation. Diazonium

salts: Preparation: from aromatic amines. Reactions: conversion to benzene, phenol, dyes.

(6 Lectures)

UNIT-IV: Amino Acids, Peptides and Proteins:

Preparation of Amino Acids: Strecker synthesis using Gabriels phthalimide synthesis.

Zwitterion,Isoelectric point and Electrophoresis. Reactions of Amino acids: ester of COOH

group, acetylation of NH2 group, complexation with Cu2+ ions, ninhydrin test.

Overview of Primary, Secondary, Tertiary and Quaternary Structure of proteins.

Determination of Primary structure of Peptides by degradation Edmann degradation

(Nterminal) and Cterminal (thio-hydantoin and with carboxypeptidase enzyme). Synthesis of

simple peptides (upto dipeptides) by N-protection (t-butyloxycarbonyl and phthaloyl) & C-

activating groups and Merrifield solid-phase synthesis. (10 Lectures).

Carbohydrates: Classification, and General Properties, Glucose and Fructose (open chain

and cyclic structure), Determinationof configuration of monosaccharides, absolute

configurationof Glucose andFructose, Mutarotation, ascendinganddescending in

monosaccharides. Structure ofdisacharrides (sucrose, cellobiose, maltose,lactose) and

polysacharrides (starch and cellulose) excluding their structure elucidation.

Reference Books: G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007).

G. W. Castellan: Physical Chemistry 4th Ed. Narosa (2004).

J. C. Kotz, P. M. Treichel, J. R. Townsend, General Chemistry, Cengage Learning India

Pvt. Ltd.:New Delhi(2009).

B. H. Mahan: University Chemistry, 3rd Edn. Narosa (1998).

R.H.Petrucci, General Chemistry, 5th Edn.,Macmillan Publishing Co.: NewYork (1985).

Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd.


Finar,I. L. Organic Chemistry (Volume 1),Dorling Kindersley (India) Pvt. Ltd. (Pearson

Education).

Finar,I. L. Organic Chemistry (Volume 2),Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

Nelson, D. L. & Cox, M. M. Lehningers Principles of Biochemistry 7th Ed., W. H. Freeman.

Berg, J. M., Tymoczko, J. L. & Stryer, L. Biochemistry 7th Ed., W. H. Freeman.

PRACTICAL: DSC-1/2/3-III(2C) LAB.


Distribution

Study of the equilibrium of one of the following reactions by the distribution method:

Conductance

I. Determination of cell constant.

II. Determination of equivalent conductance, degree of dissociation and dissociation

constant of a

weak acid.

III. Perform the following conductometric titrations:

i. Strong acid vs. strong base.

ii. Weakacid vs. strongbase.

Potentiometry Perform the following potentiometric titrations:

i. Strong acid vs. strong base.

ii. Weak acid vs. strong base.

iii. Potassium dichromate vs. Mohr's salt.


I. Systematic Qualitative Organic Analysis of Organic Compounds possessing monofunctional

groups (-COOH, phenolic, aldehydic, ketonic, amide, nitro, amines) and preparation of one

derivative.

II. Separation of amino acids by paper chromatography.

2. Determination of the concentration of glycine solution by formylation method.

3. Titration curve of glycine.

4. Action of salivary amylase on starch.

5. Effect of temperature on the action of salivary amylase on starch.

6. Differentiation between a reducing/nonreducing sugar.

Reference Books: A.I. Vogel: Textbook of Practical Organic Chemistry, Prentice Hall, 5th Edn.

F. G. Mann & B. C.Saunders: Practical OrganicChemistry, Orient Longman, 1960.

B.D. Khosla: Senior Practical Physical Chemistry, R. Chand & Co.

Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry, Universities Press.

SEMESTER-IV DSC-1/2/3-IV(2D): CHEMISTRY OFS-ANDP-BLOCK ELEMENTS,STATESOF

MATTER & CHEMICAL KINETICS

THEORY (Each class 1 hour):75 Marks [60 (Sem) +15 (Int.)]

PRACTICAL (Each class 2 hours):25 Marks

Lectures: 60(40 Theory + 20 Practical classes)

Section A: Inorganic Chemistry-2 (30 Lectures)

UNIT-I: General Principles of Metallurgy

Chief modes of occurrence of metals based on standard electrode potentials. Ellingham

diagrams for reduction of metal oxides using carbon as reducing agent. Hydrometallurgy,

Methodsofpurificationof metals(Al,Pb,Fe,Cu,Ni,Zn):electrolytic,oxidative refining,

Parting process, van Arkel-de Boer process and Monds process. (4 Lectures)

s- and p-Block Elements

Periodicityin s- andp-block elements with respect to electroniccon_guration, atomicand

ionic size, ionization enthalpy, electronegativity (Pauling & Mulliken scales). Allotropy in C, S,

andP.Oxidationstateswithreferencetoelementsinunusualandrareoxidationstateslike

carbidesandnitrides), inertpaireffect,diagonalrelationshipandanomalousbehaviourof

first member of each group. (11 Lectures).

UNIT-II: Compounds of s- and p-Block Elements

Hydrides and their classi_cation (ionic, covalent and interstitial), structure and properties

with respect tostabilityof hydrides of p- blockelements. Concept of multicentrebonding

(diborane).Structure, bonding and their important properties like oxidation/reduction,

acidic/basic nature of the following compounds and their applications in industrial, organic

and environmental chemistry. Hydrides of nitrogen(NH3;N2H4;N3H;NH2OH)

Oxoacids of P, S and Cl.

Halides and oxohalides: PCl3; PCl5; SOCl2: (15 Lectures)

Section B: Physical Chemistry-3 (30 Lectures)

UNIT-III: Kinetic Theory of Gases

Postulates of Kinetic Theory of Gases and derivation of the kinetic gas equation. Deviation of

real gases from ideal behaviour, compressibility factor, causes of deviation. van der Waals

equation of state for real gases. Boyle temperature (derivation not required). Critical

phenomena, critical constants and their calculation from van der Waals equation. Maxwell

Boltzmann distribution laws of molecular velocities and molecular energies (graphic

representation derivation not required) and their importance.

Temperaturedependence of thesedistributions. Mostprobable,averageandrootmean

square velocities (no derivation). Collision cross section, collision number, collision

frequency, collision diameter and mean free path of molecules. Viscosity of gases and effect

of temperature and pressure on coefficient of viscosity (qualitative treatment only). (10

Lectures)

Liquids

Surface tension and its determination using stalagmometer. Viscosity of a liquid and

determination of coefficient of viscosity using Ostwald viscometer. Effect of temperature on

surface tension and coefficient of viscosity of a liquid (qualitative treatment only). (5

Lectures)

UNIT-IV: Solids

Formsofsolids.Symmetryelements,unitcells,crystalsystems,Bravaislatticetypesand

identification of lattice planes. Laws of Crystallography - Law of constancy of interfacial

angles, Lawof rational indices. Millerindices. XRaydiffraction bycrystals, Braggs law.

Structuresof NaCl, and CsCl (qualitative treatment only). Defects in crystals. (7 Lectures)

Chemical Kinetics

The concept of reaction rates. Effect of temperature, pressure, catalyst and other factors on

reaction rates. Order and molecularity of a reaction. Derivation of integrated rate equations

for zero, first and second order reactions (both for equal and unequal concentrations of

reactants). Halflifeof areaction. General methodsfordeterminationoforderof areaction.

Concept of activation energy and its calculation from Arrhenius equation. Theories of

Reaction Rates: Collision theory and Activated Complex theory of bimolecular reactions.

Comparison of the two theories (qualitative treatment only).

(8 Lectures)

Reference Books: G.M.Barrow: Physical ChemistryTata McGraw-Hill(2007).

G. W. Castellan: Physical Chemistry 4th Edn. Narosa (2004).

C.Kotz,P.M.Treichel&J.R.Townsend: GeneralChemistryCengageLeningIndia Pvt. Ltd.,New Delhi(2009).

H. Mahan: University Chemistry 3rd Ed. Narosa (1998).

R.H.Petrucci:GeneralChemistry5thEd.MacmillanPublishingCo.:NewYork(1985).

D. Lee: A New Concise Inorganic Chemistry, E.L.B.S.

F.A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley.

F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press.

Gary Wulfsberg: Inorganic Chemistry, Viva Books Pvt. Ltd.

PRACTICAL: DSC-1/2/3-IV(2D) LAB.

Section A: Inorganic Chemistry

Semi-micro qualitative analysis using H2S of mixtures- not more than four ionic species (two

anions and two cations and excluding insoluble salts) out of the following:

Cations :

Actions:

(Spot tests should be carried out wherever feasible)

Section B: Physical Chemistry

Chemical Kinetics

Study the kinetics of the following reactions.

3. Initial rate method: Iodide-persulphate reaction.

4. Integrated rate method:

a) Acid hydrolysis of methyl acetate with hydrochloric acid.

b) Saponi_cation of ethyl acetate.

c) Compare the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of methyl acetate.

Reference Books: A.I. Vogel, Qualitative Inorganic Analysis, Prentice Hall, 7th Edn

A.I. Vogel, Quantitative Chemical Analysis, Prentice Hall, 6th Edn.

B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & C

Semester-V

CC-11: ORGANIC CHEMISTRY-IV (Credits-6: Theory-4, Practical-2)-Max. Marks: 100

THEORY (Each class 1 hr.): Marks-75 [60 (Sem) +15 (Int.)]



UNIT-I:Nucleic Acids

Components of nucleic acids, Nucleosides and nucleotides; Structure, synthesis and

reactions of: Adenine, Guanine, Cytosine, Uracil and Thymine; Structure of polynucleotides.

(9 Lectures)

Enzymes

Introduction, classi_cation and characteristics of enzymes. Salient features of active site of

enzymes.Mechanism of enzyme action (taking trypsin as example), factors a_ecting enzyme

action, coen-zymes and cofactors and their role in biological reactions, speci_city of enzyme

action (including stereospeci_city), enzyme inhibitors and their importance, phenomenon of

inhibition (competitive, uncompetitive and non-competitive inhibition including allosteric

inhibition). (8 Lectures)

UNIT-II: Amino Acids, Peptides and Proteins

Amino acids, peptides and their classi_cation. -Amino acids - Synthesis, ionic properties and

re-actions. Zwitterions, pKa values, isoelectric point and electrophoresis. Study of peptides:

deter-mination of their primary structures-end group analysis, methods of peptide

synthesis. Synthesis of peptides using N-protecting, C-protecting and C-activating groups -

Solid-phase synthesis (16 Lectures)

UNIT-III: Lipids

Introduction to oils and fats; common fatty acids present in oils and fats, Hydrogenntion of

fats and oils, Saponi_cation value, acid value, iodine number. Reversion and rancidity. (8

Lectures)

Concept of Energy in Biosystems

Cells obtain energy by the oxidation of foodstu_ (organic molecules). Introduction to

metabolism (catabolism and anabolism). Overview of catabolic pathways of fat and protein.

Interrelationship in the metabolic pathways of protein, fat and carbohydrate. Caloric value

of food, standard caloric

content of food types. (7 Lectures)

UNIT-IV: Pharmaceutical Compounds: Structure and Importance

Classi_cation, structure and therapeutic uses of antipyretics: Paracetamol (with synthesis),

Anal-gesics: Ibuprofen (with synthesis), Antimalarials: Chloroquine (with synthesis). An

elementary treat-ment of Antibiotics and detailed study of chloramphenicol, Medicinal

values of curcumin (haldi), azadirachtin (neem), vitamin C and antacid (ranitidine). (12

Lectures)

Reference Books:

_ Berg, J.M., Tymoczko, J.L. and Stryer, L. (2006) Biochemistry. VIth Edition. W.H. Freeman

and Co.

_ Nelson, D.L., Cox, M.M. and Lehninger, A.L. (2009) Principles of Biochemistry. IV Edition.

W.H.Freeman and Co.

_ Murray, R.K., Granner, D.K., Mayes, P.A. and Rodwell, V.W. (2009) Harpers Illustrated

Biochem-istry. XXVIII edition. Lange Medical Books/ McGraw-Hill.


1. Preparations of the following compounds:

i. Aspirine, ii. Phenacetin, iii. Milk of magnesia, iv. Aluminium hydroxide gel, v. Divol.

2. Saponi_cation value of an oil or a fat.

3. Determination of Iodine number of an oil/ fat.

Reference Books: _ Manual of BiochemistryWorkshop, 2012, Department of Chemistry, University of Delhi.

_ Arthur, I. Vogel, Quantitative Organic Analysis, Pearson.

Semester-V

CC-12: PHYSICAL CHEMISTRY-V (Credits-6: Theory-4, Practical-2)-Max. Marks: 100




UNIT-I: Quantum Chemistry

Postulates of quantum mechanics, quantum mechanical operators, Schrdinger equation and

its ap-plication to free particle and particle-in-a-box (rigorous treatment), quantization of

energy levels, zero-point energy and Heisenberg Uncertainty principle; wave functions,

probability distribution functions, nodal properties. Extension to three dimensional boxes,

separation of variables, degener-

acy. Qualitative treatment of simple harmonic oscillator model of vibrational motion:

Setting up of Schrdinger equation and discussion of solution and wave functions. Vibrational

energy of diatomic molecules and zero-point energy. Angular momentum: Commutation

rules, quantization of square of total angular momentum and z-component. Rigid rotator

model of rotation of diatomic molecule. Schrdinger equation, transformation to spherical

polar coordinates. Separation of variables (Prelim-inary treatment). Qualitative treatment of

hydrogen atom and hydrogen-like ions: setting up of Schrdinger equation in spherical polar

coordinates, radial part, quantization of energy (only _nal energy expression). Average and

most probable distances of electron from nucleus. (18 Lectures)

UNIT-II: Chemical Bonding

Chemical bonding: Covalent bonding, valence bond and molecular orbital approaches,

LCAO-MO treatment of H+ 2 : Bonding and antibonding orbitals. Qualitative extension to H2:

Comparison of LCAO-MO and VB treatments of H2 (only wavefunctions, detailed solution not

required) and their limitations. Qualitative description of LCAO-MO treatment of

homonuclear and heteronuclear diatomic molecules (HF, LiH). Localised and non-localised

molecular orbitals treatment of triatomic (BeH2, H2O) molecules. Qualitative MO theory

and its application to AH2 type molecules. (12 Lectures)

UNIT-III: Molecular Spectroscopy-I

Interaction of electromagnetic radiation with molecules and various types of spectra; Born-

Oppenheimer approximation. Rotation spectroscopy: Selection rules, intensities of spectral

lines, determination of bond lengths of diatomic and linear triatomic molecules, isotopic

substitution. Vibrational spectroscopy: Classical equation of vibration, computation of force

constant, amplitude of diatomic molecular vibrations, anharmonicity, Morse potential,

dissociation energies, fundamental frequencies, overtones, hot bands, degrees of freedom

for polyatomic molecules, modes of vibration. Vibration-rotation spectroscopy: diatomic

vibrating rotator, P, Q, R branches. Raman spectroscopy: Qualitative treatment of Rotational

Raman e_ect; E_ect of nuclear spin, Vibrational Raman spectra, Stokes and anti-Stokes lines;

their intensity di_erence, rule of mutual exclusion. (16 Lectures)

UNIT-IV: Molecular Spectroscopy-II

Electronic spectroscopy: Franck-Condon principle, electronic transitions, singlet and triplet

states, uorescence and phosphorescence, dissociation and predissociation. (6 Lectures)

Photochemistry

Characteristics of electromagnetic radiation, Lambert-Beers law and its limitations, physical

signi_-cance of absorption coe_cients. Laws, of photochemistry, quantum yield,

actinometry, examples of low and high quantum yields, photochemical equilibrium and the

di_erential rate of photochemical reactions, photosensitised reactions, quenching. Role of

photochemical reactions inbiochemical

processes, photostationary states, chemiluminescence. (8 Lectures)

Reference Books: _ Banwell, C. N. & McCash, E. M. Fundamentals of Molecular Spectroscopy 4th Ed. Tata

McGraw-Hill: New Delhi(2006).

_ Chandra, A. K. Introductory Quantum Chemistry Tata McGraw-Hill (2001).

_ House, J. E. Fundamentals of Quantum Chemistry 2nd Ed. Elsevier: USA (2004).

_ Lowe, J. P. & Peterson, K. Quantum Chemistry, Academic Press (2005).

_ Kakkar, R. Atomic & Molecular Spectroscopy, Cambridge University Press (2015).


Colourimetry

1. Determine the concentration of HCl against 0.1 N NaOH spectrophotometrically. 2. To

_nd the strength of given ferric ammonium sulfate solution of (0.05 M) by using EDTA

spectrophotometrically.

3. To_ndoutthestrength of CuSO4solutionbytitratingwithEDTA spectrophotometrically.

4. To determine the concentration of Cu(II) and Fe(III) solution photometrically by titrating

with EDTA.

Reference Books: _ Khosla, B. D.; Garg, V. C. & Gulati, A., Senior Practical Physical Chemistry, R. Chand &

Co.:New Delhi (2011).

_ Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry 8th Ed.;

McGraw-Hill: New York (2003).

_ Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H. Freeman &

Co.: New York (2003).

_ Experimental Physical Chemistry by J. N. Gurtu, R. Kapoor.

Semester-V

DISCIPLINE SPECIFIC ELECTIVE (DSE) SEMESTER-V

DSE-1: POLYMER CHEMISTRY





UNIT-I: Introduction and history of polymeric materials:

Di_erent schemes of classi_cation of polymers, Polymer nomenclature, Molecular forces

and chemical bonding in polymers, Texture of Polymers. (4 Lectures)

Functionality and its importance:

Criteria for synthetic polymer formation, classi_cation of polymerization processes,

Relationshipsbetween functionality, extent of reaction and degree of polymerization. Bi-

functional systems, Poly-functional systems. (8 Lectures)

UNIT-II: Kinetics of Polymerization:

Mechanism and kinetics of step growth, radical chain growth, ionic chain (both cationic and

anionic) and coordination polymerizations, Mechanism and kinetics of copolymerization,

polymerization tech-niques. (8lectures)

Crystallization and crystallinity:

Determination of crystalline melting point and degree of crystallinity, Morphology of

crystalline poly-mers, Factors a_ecting crystalline melting point. (4 Lectures)

Nature and structure of polymers-Structure property relationships. (2 Lectures)

UNIT-III: Determination of molecular weight of polymers

(Mn, Mw, etc.) by end group analysis, viscometry, light scattering and osmotic pressure

methods.Molecular weight distribution and its signi_cance. Polydispersity index. (8 Lectures) Glass transition temperature (Tg) and determination of Tg

WLF equation, Factors a_ecting glass transition temperature (Tg). (8 Lectures)

UNIT-IV: Polymer Solution

Criteria for polymer solubility, Solubility parameter, Thermodynamics of polymer solutions,

entropy,enthalpy, and free energy change of mixing of polymers solutions. (8 Lectures)

Properties of Polymers

(Physical, thermal & mechanical properties). Brief introduction to preparation, structure,

prop-erties and application of the following polymers: polyole_ns, polystyrene and styrene

copolymers,

poly(vinyl chloride) poly(vinyl acetate), polyacrylamide, uoro polymers (Teon), polyamides

(nylon-6 and nylon 6,6). Phenol formaldehyde resins (Bakelite, Novalac), polyurethanes,

silicone polymers (polysiloxane), Polycarbonates, Conducting Polymers, (polyacetylene,

polyaniline). (10 Lectures)

Reference Books: _ Seymours Polymer Chemistry, Marcel Dekker, Inc.

_ G. Odian: Principles of Polymerization, John Wiley.

_ F.W. Billmeyer: Text Book of Polymer Science, John Wiley.

_ P. Ghosh: Polymer Science & Technology, Tata Mcgraw-Hill.

_ R.W. Lenz: Organic Chemistry of Synthetic High Polymers.

PRACTICAL: DSE-1 LAB.

Polymer synthesis

1. Free radical solution polymerization of styrene (St) / Methyl Methacrylate (MMA) /

Methyl Acrylate (MA) / Acrylic acid (AA).

(a) Puri_cation of monomer.

(b) Polymerization using benzoyl peroxide (BPO) / 2,2-azo-bis-isobutylonitrile (AIBN).

2. Preparation of nylon 66/6.

3. Interfacial polymerization, preparation of polyester from isophthaloyl chloride (IPC) and

phe-nolphthalein.

(a) Preparation of IPC.

(b) Puri_cation of IPC.

(c) Interfacial polymerization.

4. Redox polymerization of acrylamide.

5. Precipitation polymerization of acrylonitrile.

6. Preparation of urea-formaldehyde resin.

7. Preparations of novalac resin/resold resin.

8. Microscale Emulsion Polymerization of poly(methylacrylate).

Polymer characterization

1. Determination of molecular weight by viscometry:

(a) Polyacrylamide-aq. NaNO2 solution

(b) (Poly vinyl proplylidine (PVP) in water

2. Determination of the viscosity-average molecular weight of poly(vinyl alcohol) (PVOH)

and the fraction of head-to-head monomer linkages in the polymer.

3. Determination of molecular wt. by end group analysis: Polyethylene glycol (PEG) (OH

group).

4. Determination of hydroxyl number of a polymer using colorimetric method.

Polymer analysis

1. Estimation of the amount of HCHO in the given solution by sodium sulphite method

2. Instrumental Techniques

3. IR studies of polymers

*at least 5 experiments to be carried out.

Reference Books: _ Malcohm P. Stevens, Polymer Chemistry: An Introduction, 3rd Ed.

_ Harry R. Allcock, Frederick W. Lampe and James E. Mark, Contemporary Polymer

Chemistry, 3rd ed. Prentice-Hall (2003).

_ Fred W. Billmeyer, Textbook of Polymer Science, 3rd ed. Wiley-Interscience (1984).

_ Joel R. Fried, Polymer Science and Technology, 2nd ed. Prentice-Hall (2003).

_ Petr Munk and Tejraj M. Aminabhavi, Introduction to Macromolecular Science, 2nd ed.

John Wiley & Sons (2002).

_ L.H. Sperling, Introduction to Physical Polymer Science, 4th ed. John Wiley & Sons (2005).

_ Malcolm P. Stevens, Polymer Chemistry: An Introduction, 3rd ed. Oxford University Press

(2005).

_ Seymour/ Carrahers Polymer Chemistry, 9th ed. by Charles E. Carraher, Jr. (2013).

Semester-V

DISCIPLINE SPECIFIC ELECTIVE (DSE) DSE-2: GREEN CHEMISTRY





UNIT-I: Introduction to Green Chemistry

What is Green Chemistry? Need for Green Chemistry. Goals of Green Chemistry.

Limitations/Obstacles in the pursuit of the goals of Green Chemistry. (4 Lectures)

Principles of Green Chemistry and Designing a Chemical synthesis-I

Twelve principles of Green Chemistry with their explanations and examples with special

emphasis on: Designing a Green Synthesis using these principles; Prevention of Waste/

byproducts; maximum incorporation of the materials used in the process into the _nal

products, Atom Economy, calculation of atom economy of the rearrangement, addition,

substitution and elimination reactions. Prevention/minimization of hazardous/ toxic

products reducing toxicity. risk = (function) hazard exposure; waste or pollution prevention

hierarchy. Green solvents supercritical uids, water as a solvent for organic reactions, ionic

liquids, uorous biphasic solvent, PEG, solventless processes, immobilized solvents and how

to compare greenness of solvents. (12 Lectures)

UNIT-II: Principles of Green Chemistry and Designing a Chemical synthesis-II

Explanation of principles with special emphasis on: Energy requirements for reactions

alterna-tive sources of energy: use of microwaves and ultrasonic energy. Selection of

starting materials; avoidance of unnecessary derivatization careful use of

blocking/protecting groups. Use of catalytic reagents (wherever possible) in preference to

stoichiometric reagents; catalysis and green chemistry, comparison of heterogeneous and

homogeneous catalysis, biocatalysis, asymmetric catalysis and photocatalysis. Prevention of

chemical accidents designing greener processes, inherent safer design, principle of ISD What

you dont have cannot harm you, greener alternative to Bhopal Gas Tragedy (safer route to

carcarbaryl) and Flixiborough accident (safer route to cyclohexanol) subdivision of ISD,

minimization, simpli_cation, substitution, moderation and limitation. Strengthening/

develop-ment of analytical techniques to prevent and minimize the generation of hazardous

substances in chemical processes. (14 Lectures)

UNIT-III: Examples of Green Synthesis/ Reactions and some real world cases-I

Green Synthesis of the following compounds: adipic acid, catechol, disodium iminodiacetate

(alter-native to Strecker synthesis) Microwave assisted reactions in water: Hofmann

Elimination, methyl benzoate to benzoic acid, oxidation of toluene and alcohols; microwave

assisted reactions in organic solvents: Diels-Alder reaction and Decarboxylation reaction.

Ultrasound assisted reactions: sonochemical Simmons-Smith Reaction (Ultrasonic

alternative to Iodine). Surfactants for carbon dioxide replacing smog producing and ozone

depleting solvents with CO2 for precision cleaning and dry cleaning of garments. Designing

of Environmentally safe marine antifoulant. (14 Lectures)

UNIT-IV: Examples of Green Synthesis/ Reactions and some real world cases-II

Right_t pigment: synthetic azopigments to replace toxic organic and inorganic pigments. An

ecient, green synthesis of a compostable and widely applicable plastic (poly lactic acid)

made from corn. Healthier Fats and oil by Green Chemistry: Enzymatic Inter esteri_cation

for production of no Trans-Fats and Oils Development of Fully Recyclable Carpet: Cradle to

Cradle Carpeting (6 Lectures)

Future Trends in Green Chemistry

Oxidation reagents and catalysts; Biomimetic, multifunctional reagents; Combinatorial

green chem-

istry; Proliferation of solventless reactions; co crystal controlled solid state synthesis (C2S3);

Green chemistry in sustainable development. (10 Lectures)

Reference Books: _ V.K. Ahluwalia & M.R. Kidwai: New Trends in Green Chemistry, _ Anamalaya Publishers

(2005).

_ P.T. Anastas & J.K. Warner: Oxford Green Chemistry- Theory and Practical, University Press

(1998).

_ A.S. Matlack: Introduction to Green Chemistry, Marcel Dekker (2001).

_ M.C. Cann & M.E. Connely: Real-World cases in Green Chemistry, American Chemical

Society, Washington (2000).

_ M.A. Ryan & M. Tinnesand, Introduction to Green Chemistry, American Chemical Society,

Wash-ington (2002).

PRACTICAL: DSE-2

1. Safer starting materials.

_ The Vitamin C clock reaction using Vitamin C tablets, tincture of iodine, hydrogen peroxide

and liquid laundry starch.

_ E_ect of concentration on clock reaction.

_ Preparation and characterization of nanoparticles (Ag, Au) using plant extract.

2. Using renewable resources

_ Preparation of biodiesel from vegetable oil.

3. Avoiding waste

_Principle of atom economy.

_ Use of molecular model kit to stimulate the reaction to investigate how the atom

economy can

illustrate Green Chemistry.

_ Preparation of propene by two methods can be studied.

(I) Triethylamine ion + OH H2SO4=4 propene + trimethylpropene + water

(II) 1-propanol ! propene + water

_ The other types of reactions, like addition, elimination, substitution and rearrangement

should also be studied for the calculation of atom economy. 4. Use of enzymes as catalysts

_ Benzoin condensation using Thiamine Hydrochloride as a catalyst instead of cyanide

4. Alternative Green solvents

Diels Alderreaction in water

_ Reaction between furan and maleic acid in water and at room temperature rather than in

benzene

and reux.

_ Extraction of D-limonene from orange peel using liquid CO2 prepared form dry ice.

_ Mechanochemical solvent free synthesis of azomethines

5. Alternative sources of energy

_Solventfree,microwave assistedonepotsynthesisofphthalocyaninecomplexof Cu(II).

_Photoreduction of benzophenone to benzopinacol in the presence of sunlight.

Reference Books: _ Anastas, P.T & Warner, J.C. Green Chemistry: Theory and Practice, Oxford University Press

(1998).

_ Kirchoff, M. & Ryan, M.A. Greener approaches to undergraduate chemistry experiment.

American Chemical Society, Washington DC (2002).

_ Ryan, M.A. Introduction to Green Chemistry, Tinnesand; (Ed), American Chemical Society,

Wash-ington DC (2002).

_ Sharma, R.K.; Sidhwani, I.T. & Chaudhari, M.K. I.K. Green Chemistry Experiment: A

monograph International Publishing House Pvt Ltd. New Delhi. Bangalore CISBN 978-93-

81141-55-7 (2013).

_ Cann, M.C. & Connelly, M. E. Real world cases in Green Chemistry, American Chemical

Society (2008).

_ Cann, M. C. & Thomas, P. Real world cases in Green Chemistry, American Chemical Society

(2008).

Chem. SEC-III (For Gen.) OF SEM-V IS SAME AS OF Chem. SEC-II OF SEM-IV (For Hons) Chem. DSE-A/B/C-I (For Gen.) OF SEM-V I IS SAME AS OF Chem. DSE-I OF SEM-V (For Hons)

SEMESTER- VI

CC-13: INORGANIC CHEMISTRY-IV





UNIT-I: Organometallic Compounds-I

De_nition and classi_cation of organometallic compounds on the basis of bond type.

Concept of hapticity of organic ligands. Metal carbonyls: 18 electron rule, electron count of

mononuclear, polynuclear and substituted metal carbonyls of 3d series. General methods of

preparation (direct combination, reductive carbonylation, thermal and photochemical

decomposition) of mono and binuclear carbonyls of 3d series. Structures of mononuclear

and binuclear carbonyls of Cr, Mn, Fe, Co and Ni using VBT. -acceptor behaviour of CO (MO

diagram of CO to be discussed), synergic effect and use of IR data to explain extent of back

bonding. Zeises salt: Preparation and structure, evidences of synergic e_ect and comparison

of synergic e_ect with that in carbonyls. (14 Lectures)

UNIT-II: Organometallic Compounds-II

Metal Alkyls: Important structural features of methyl lithium (tetramer) and trialkyl

aluminium (dimer), concept of multicentre bonding in these compounds. Role of

triethylaluminium in poly-merisation of ethene (Ziegler Natta Catalyst). Species present in

ether solution of Grignard reagent and their structures. Ferrocene: Preparation and

reactions (acetylation, alkylation, metallation, Mannich Condensation), structure and

aromaticity, comparison of aromaticity and reactivity with that of benzene. (14 Lectures)

UNIT-III: Theoretical Principles in Qualitative Analysis (H2S Scheme)

Basic principles involved in analysis of cations and anions and solubility products, common

ion e_ect. Principles involved in separation of cations into groups and choice of group

reagents. Interfering anions (uoride, borate, oxalate and phosphate) and need to remove

them after Group II. (10 Lectures)

Catalysis by Organometallic Compounds

Study of the following industrial processes and their mechanism:

1. Alkene hydrogenation (Wilkinsons Catalyst).

2. Hydroformylation (Co salts).

3. Wacker Process.

4. Synthetic gasoline (Fischer Tropsch reaction). (8 Lectures)

UNIT-IV: Reaction Kinetics and Mechanism

Introduction to inorganic reaction mechanisms. Substitution reactions in square planar

complexes, Trans-e_ect and its applications, theories of trans e_ect, Mechanism of

nucleophilic substitution in square planar complexes. Thermodynamic and kinetic stability,

Kinetics of octahedral substitution (classi_cation of metal ions based on water exchange

rate), General mechanism of substitution in

octahedral complexes (D, I, Id, Ia). (14 Lectures)

Reference Books: _ Vogel, A.I. Qualitative Inorganic Analysis, Longman, 1972.

_ Svehla, G. Vogel's Qualitative Inorganic Analysis, 7th Edition, Prentice Hall, 1996-03-07.

_ Huheey, J. E.; Keiter, E.A. & Keiter, R.L. Inorganic Chemistry, Principles of Structure and

Reac-tivity 4th Ed., Harper Collins 1993, Pearson,2006.

_ Sharpe, A.G. Inorganic Chemistry, 4th Indian Reprint (Pearson Education) 2005.

_ Douglas, B. E.; McDaniel, D.H. & Alexander, J.J. Concepts and Models in Inorganic

Chemistry, 3rd Ed., John Wiley and Sons, NY, 1994.

_ Greenwood, N.N. & Earnshaw, A. Chemistry of the Elements, Elsevier 2nd Ed, 1997 (Ziegler

Natta Catalyst and Equilibria in Grignard Solution).

_ Lee, J.D. Concise Inorganic Chemistry 5th Ed., John Wiley and sons 2008.

_ Powell, P. Principles of Organometallic Chemistry, Chapman and Hall, 1988.

_ Shriver, D.D. & P. Atkins, Inorganic Chemistry 2nd Ed., Oxford University Press, 1994.

_ Basolo, F. & Person, R. Mechanisms of Inorganic Reactions: Study of Metal Complexes in

Solution 2nd Ed., John Wiley & Sons Inc; NY.

_ Purcell, K.F. & Kotz, J.C., Inorganic Chemistry, W.B. Saunders Co. 1977.

_ Miessler, G. L. & Donald, A. Tarr, Inorganic Chemistry 4th Ed., Pearson, 2010.

_ Collman, James P. et al. Principles and Applications of Organotransition Metal Chemistry.

Mill Valley, CA: University Science Books, 1987.

_ Crabtree, Robert H. The Organometallic Chemistry of the Transition Metals, New York, NY:

John Wiley, 2000.

_ Spessard, Gary O., & Gary L. Miessler. Organometallic Chemistry. Upper Saddle River, NJ:

Prentice-Hall, 1996.

_ Mehrotra R.C. and Singh, A. Organometallic Chemistry, New Age International Publishers,

2nd Edn, 2000.

PRACTICAL: C-13 LAB.

Qualitative semimicro analysis of mixtures containing 3 anions and 3 cations. Emphasis

should be given to the understanding of the chemistry of di_erent reactions. The following

radicals are

suggested:

CO23 ;NO2 ; S; SO3 ; S2O23 ;CH3COO; F;Cl;Br; I;NO3 ;BO3 ;C2O24 ; PO34;NH+4;K+;

Pb+2;Cu+2;Cd+2;Bi+3;Sn2+;Sb3+;Fe3+;Al3+; ;Cr3+;Zn2+;Mn2+;Co2+;Ni2+;Ba2+; Sr2+;Ca2+;Mg2+: Mixtures

should preferably contain one interfering anion, or insoluble component(BaSO4; SrSO4;

PbSO4;CaF2orAl2O3) or combination of anions e.g. CO2

3 and SO23 ;NO2and NO3;Cl and Br;Cl and I;Br and I;NO3 and Br;NO3 and I: Spot test should

be done whenever possible.

Reference Books:

_ Vogels Qualitative Inorganic Analysis, Revised by G. Svehla.

_ Marr & Rockett Inorganic Preparations.

SEMESTER- VI

CC-14: ORGANIC CHEMISTRY-IV (Credits-6: Theory-4, Practical-2)-Max. Marks: 100



Lectures: 60 (40 Theory + 20 Practical classes) Lectures: 60(40 Theory + 20 Practical classes)

UNIT-I: Organic Spectroscopy-I

UV Spectroscopy: Types of electronic transitions, max, Chromophores and Auxochromes,

Bathochromic and Hypsochromic shifts, Intensity of absorption; Application of Woodward

rules for calculation of max for the following systems: , the unsaturated aldehydes: ketones,

carboxylic acids and esters;Conjugated dienes: alicyclic, homoannular and heteroannular;

Extended conjugated systems (alde-hydes, ketones and dienes); distinction between cis and

trans isomers.IR Spectroscopy: Fundamental and non-fundamental molecular vibrations; IR

absorption positionsof O, N and S containing functional groups; E_ect of H-bonding,

conjugation, resonance and ring size on IR absorptions; Fingerprint region and its

signi_cance; application in functional group analysis. (18 Lectures)

UNIT-II: Organic Spectroscopy-II

NMR Spectroscopy: Basic principles of Proton Magnetic Resonance, chemical shift and

factors inuencing it; Spin-spin coupling and coupling constant; Anisotropic e_ects in alkene,

alkyne, alde-hydes and aromatics; Interpretation of NMR spectra of simple compounds.

Mass Spectroscopy-Basic principle, Fragmentation pattern, Instrumentation, Determination

of m/e ratio. Application of Mass Spectroscopy on CH4, C2H6, n-butane and neo-pentane.

Applications of IR, UV and NMR for identi_cation of simple organic molecules. (12 Lectures)

UNIT-III: Carbohydrates

Occurrence, classi_cation and their biological importance. Monosaccharides: Constitution

and abso-lute con_guration of glucose and fructose, epimers and anomers, mutarotation,

determination of ring size of glucose and fructose, Haworth projections and conformational

structures; Interconversions of aldoses and ketoses; Killiani-Fischer synthesis and Ru_

degradation; Disaccharides Structure elucidation of maltose. Polysaccharides Elementary

treatment of starch, cellulose. (8 Lectures)

Dyes

Classi_cation, colour and constitution; Mordant and Vat dyes; Chemistry of dyeing.

Synthesis and applications of: Azo dyes Methyl orange and Congo red (mechanism of Diazo

Coupling); Triphenyl methane dyes - Malachite Green, and crystal violet; Phthalein dyes

Phenolphthalein and Fluorescein; Natural dyes Alizarin and Indigo; Edible dyes with

examples. (8 Lectures)

UNIT-IV: Polymers

Introduction and classi_cation including di-block, tri-block and amphiphilic polymers;

Number av-erage molecular weight, Weight average molecular weight, Degree of

polymerization, Polydispersity Index. Polymerisation reactions -Addition and condensation -

Mechanism of cationic, anionic and free radical addition polymerization; Metallocene-based

Ziegler-Natta polymerisation of alkenes; Preparation and applications of plastics

thermosetting (phenol-formaldehyde, Polyurethanes) and thermosoftening (PVC,

polythene); Fabrics natural and synthetic (acrylic, polyamido, polyester); Rubbers natural

and synthetic: Buna-S and Neoprene; Vulcanization; Polymer additives; Biodegrad-able and

conducting polymers with examples. (14 Lectures)

Reference Books: _ Kalsi, P. S. Textbook of Organic Chemistry 1st Ed., New Age International (P) Ltd. Pub.

_ Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd.


_ Billmeyer, F. W. Textbook of Polymer Science, John Wiley & Sons, Inc.

_ Gowariker, V. R.; Viswanathan, N. V. & Sreedhar, J. Polymer Science, New Age

International (P) Ltd. Pub.

_ Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural

Prod-ucts), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

_ Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc.

_ Clayden, J.; Greeves, N.; Warren, S.; Wothers, P.; Organic Chemistry, Oxford University

Press.

_Singh, J.; Ali, S.M. & Singh, J. Natural Product Chemistry, Pragati Prakashan (2010).

_ Kemp, W. Organic Spectroscopy, Palgrave.


1. Extraction of ca_eine from tea leaves.

2. Preparation of sodiumpolyacrylate.

3. Preparation of ureaformaldehyde.

4. Analysis of Carbohydrate: aldoses and ketoses, reducing and non-reducing sugars.

5. Qualitative analysis of unknown organic compounds containing mono-functional groups

(car-bohydrates, aryl halides, aromatic hydrocarbons, nitro compounds, amines and amides)

and simple bifunctional groups, for e.g. salicylic acid, cinnamic acid, nitrophenols etc.

Reference Books: _ Vogel, A.I. Quantitative Organic Analysis, Part 3, Pearson (2012).

_Mann,F.G.&Saunders, B.C.PracticalOrganicChemistry,Pearson Education(2009).

_ Furniss, B.S., Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic Chemistry, 5th

Ed., Pearson (2012).

_ Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry: Preparation

and Quantitative Analysis, University Press (2000).

_ Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic Chemistry: Qualitative


SEMESTER- VI

DISCIPLINE SPECIFIC ELECTIVE (DSE) DSE-3: INDUSTRIAL CHEMICALS AND ENVIRONMENT





UNIT-I: Industrial Gases and Inorganic Chemicals

Industrial Gases: Large scale production, uses, storage and hazards in handling of the

following gases: oxygen, nitrogen, argon, neon, helium, hydrogen, acetylene, carbon

monoxide, chlorine, sul-phur dioxide. Inorganic Chemicals: Manufacture, application and

hazards in handling the following chemicals: hydrochloric acid, nitric acid, sulphuric acid,

caustic soda, common salt, bleaching pow-der, sodium thiosulphate, hydrogen peroxide,

potash alum, potassium dichromate and potassium

permanganate. (10 Lectures)

bf Industrial Metallurgy

Preparation of metals (ferrous and nonferrous) and ultrapure metals for semiconductor

technology. (4 Lectures)

UNIT-II: Environment and its segments

Ecosystems. Biogeochemical cycles of carbon, nitrogen and sulphur. Air Pollution: Major

regions of atmosphere. Chemical and photochemical reactions in atmosphere. Air

pollutants: types, sources, particle size and chemical nature; Photochemical smog: its

constituents and photochemistry. Envi-ronmental e_ects of ozone. Major sources of air

pollution. Pollution by SO2;CO2;CO;NOx; andH2S and control procedures. E_ects of air

pollution on living organisms and vegetation. Greenhouse e_ect. and global warming, Ozone

depletion by oxides of nitrogen, chlorouorocarbons and halogens, re-moval of sulphur from

coal. (14 Lectures)

UNIT-III: Water Pollution:

Hydrological cycle, water resources, aquatic ecosystems, Sources and nature of water

pollutants, Techniques for measuring water pollution, Impacts of water pollution on

hydrological and ecosystems. Water puri_cation methods. E_uent treatment plants

(primary, sec-ondary and tertiary treatment). Industrial e_uents from the following

industries and their treatment: electroplating, textile, tannery, dairy, petroleum and

petrochemicals, fertilizer. Sludge disposal. In-dustrial waste management, incineration of

waste. Water treatment and puri_cation (reverse osmo-

sis, ion exchange). Water quality parameters for wastewater, industrial water and domestic

water. (16 Lectures)

UNIT-IV: Energy & Environment

Sources of energy: Coal, petrol and natural gas. Nuclear fusion/_ssion, solar energy,

hydrogen, geothermal, tidal and hydel. Nuclear Pollution: Disposal of nuclear waste, nuclear

disaster and its management. (10 Lectures)

Biocatalysis: Introduction to biocatalysis: Importance in green chemistry and chemical

industry. (6 Lectures)

Reference Books: _ E. Stocchi: Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK.

_ R.M. Felder, R.W. Rousseau: Elementary Principles of Chemical Processes, Wiley

Publishers, New Delhi.

_ A. Kent: Riegels Handbook of Industrial Chemistry, CBS Publishers, New Delhi.

_ S.S. Dara:ATextbookof Engineering Chemistry, S. Chand & CompanyLtd. NewDelhi.

_ De, Environmental Chemistry: New Age International Pvt., Ltd, New Delhi.

_ S. M. Khopkar, Environmental Pollution Analysis: Wiley Eastern Ltd, New Delhi.

_ S.E. Manahan, Environmental Chemistry, CRC Press (2005).

_ G.T. Miller, Environmental Science 11th edition. Brooks/ Cole (2006).

_ Mishra, Environmental Studies. Selective and Scienti_c Books, New Delhi (2005).

PRACTICAL: DSE-3

1. Determination of dissolved oxygen in water.

2. Determination of Chemical Oxygen Demand (COD).

3. Determination of Biological Oxygen Demand (BOD).

4. Percentage of available chlorine in bleaching powder.

5. Measurement of chloride, sulphate and salinity of water samples by simple titration

method (AgNO3 and potassium chromate).

6. Estimation of total alkalinity of water samples (CO2

3 ;HCO

3 ) using double titration method.

7. Measurement of dissolved CO2: 8. Study of some of the common bio-indicators of

pollution.

9. Estimation of SPM in air samples.

10. Preparation of borax/ boric acid.

Reference Books: _ E. Stocchi: Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK.

_ R.M. Felder, R.W. Rousseau: Elementary Principles of Chemical Processes, Wiley

Publishers, New Delhi.

_ A. Kent: Riegels Handbook of Industrial Chemistry, CBS Publishers, New Delhi.

_ S.S. Dara: ATextbookof Engineering Chemistry, S. Chand &CompanyLtd. NewDelhi.

_ De, Environmental Chemistry: New Age International Pvt., Ltd, New Delhi.

_ S. M. Khopkar, Environmental Pollution Analysis: Wiley Eastern Ltd, New Delhi.

SEMESTER- VI

DISCIPLINE SPECIFIC ELECTIVE (DSE) DSE-4

Dissertation: 60 Marks Presentation: 25 Marks

Viva-voce: 15 Marks

Projects submitted by the student are to be evaluated by the Internal Examiner

and External Examiner appointed by University. Students should opt for

Supervision of Dissertation from the internal faculties of his own

college/Institution. The Supervisor in consultation with the concerned Head of

the Department should decide the topic. The presentation should be open to all

faculties as well as graduate students of the concerned Department

SEMESTER- VI

SEC-IV: FUEL CHEMISTRY

(Credits: 02)- Max. Marks: 50[40 (Sem) +10 (Int.)]

30 Lectures( Each Lecture 1 hr.)

Review of energy sources (renewable and non-renewable). Classi_cation of fuels and their

calorific value Coal: Uses of coal (fuel and non-fuel) in various industries, its composition,

carbonization of coal. Coal gas, producer gas and water gascomposition and uses.

Fractionation of coal tar, uses of coal tar bases chemicals, requisites of a good metallurgical

coke, Coal gasi_cation (Hydro gasi_cation and Catalytic gasi_cation), Coal liquefaction and

Solvent Re_ning. Petroleum and Petrochemical Industry: Composition of crude petroleum,

Re_ning and di_erent types of petroleum products and their applications. Fractional

Distillation (Principle and process), Cracking (Thermal and catalytic cracking), Reforming

Petroleum and non-petroleum fuels (LPG, CNG, LNG, bio-gas, fuels derived from biomass),

fuel from waste, synthetic fuels (gaseous and liquids), clean fuels. Petrochemicals: Vinyl

acetate, Propylene oxide, Isoprene, Butadiene, Toluene and its derivatives Xylene.

Lubricants: Classi_cation of lubricants, lubricating oils (conducting and non-conducting) Solid

and semisolid lubricants, synthetic lubricants. Properties of lubricants (viscosity index, cloud

point, pore point) and their determination.

large Reference Books:

_ E. Stocchi: Industrial Chemistry, Vol -I, Ellis Horwood Ltd. UK.

_ P.C. Jain, M. Jain: Engineering Chemistry, Dhanpat Rai & Sons, Delhi.

_ B.K. Sharma: Industrial Chemistry, Goel Publishing House, Meerut. Chem. DSE-A/B/C-II (For Gen.) OF SEM-VI IS SAME AS OF Chem. DSC-III OF SEM-VI (For Hons)

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